Chem 1 CP Final Exam Study Guide by aus20718

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									Chem 1 CP Final Exam Study Guide

Multiple Choice.

   1.   What is the relative mass of an electron?
        a. 1/1840 the mass of a C-12 atom                          c.   1/1840 the mass of a neutron + proton
        b. 1/1840 the mass of an alpha particle                    d.   1/1840 the mass of a hydrogen atom

   2.   Particles in a gas are best described as ____.
        a. spheres that are in fixed positions when trapped in a container
        b. hard spheres influenced by repulsive forces from other spheres
        c. slow-moving, kinetic, hard spheres
        d. small, hard spheres with insignificant volumes

   3.   Which law can be used to calculate the number of moles of a contained gas?
        a. Charles’s law                                        c. Boyle’s law
        b. ideal gas law                                        d. combined gas law

   4.   If a balloon is squeezed, what happens to the pressure of the gas inside the balloon?
        a. It increases.
        b. The pressure depends on the type of gas in the balloon.
        c. It stays the same.
        d. It decreases.

   5.   The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation?
        a.                                                     c.
            1.54 10        m                                         1.54 10 m
        b.                                                     d.
            1.54 10 m                                                1.54 10       m

   6.   Which of the following elements has the ability to undergo sublimation?
        a. iodine                                                 c. oxygen
        b. sodium                                                 d. carbon

   7.   When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.
        a. prefix                                                c. Roman numeral following the name
        b. suffix                                                d. superscript after the name

   8.   What is the name of the ionic compound formed from lithium and bromine?
        a. lithium bromine                                      c. lithium bromium
        b. lithium bromide                                      d. lithium bromate

   9.   According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
        a. pairs of valence electrons                           c. inner shell electrons
        b. mobile electrons                                     d. the electrons closest to the nuclei

  10.   What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
        a. 4s                                                         c. 2d
        b. 3f                                                         d. 3d

  11.   What is another name for the transition metals?
        a. Group B elements                                        c.   noble gases
        b. Group A elements                                        d.   Group C elements

  12.   What is the SI unit of pressure?
        a. newton                                                  c.   pascal
        b. candela                                                 d.   mole
  13.   What is the correct name for the N    ion?
        a. nitrite ion                                             c.   nitrate ion
        b. nitride ion                                             d.   nitrogen ion

  14.   Which of the forces of molecular attraction is the weakest?
        a. dispersion                                              c.   single covalent bond
        b. hydrogen bond                                           d.   dipole interaction

  15.   What particle is emitted in alpha radiation?
        a. electron                                                c.   photon
        b. helium nucleus                                          d.   hydrogen nucleus

  16.   How many valence electrons are in an atom of phosphorus?
        a. 2                                                   c.       3
        b. 4                                                   d.       5
17.   Which of the following compounds contains the lead(II) ion?
      a. PbCl4                                                 c.       Pb2S
      b. Pb2O                                                  d.       PbO

18.   What element has the electron configuration 1s 2s 2p 3s 3p ?
      a. silver                                              c. silicon
      b. nitrogen                                            d. selenium

19.   Density is found by dividing ____.
      a. mass by area                                              c.   mass by volume
      b. volume by mass                                            d.   area by mass

20.   Which of the following compounds has the formula KNO ?
      a. potassium nitrate                                 c.           potassium nitrite
      b. potassium nitride                                 d.           potassium nitrogen oxide

21.   What particle is needed to complete this nuclear reaction?
           Rn       Po + _____
      a.                           b.                              c.                            d
                e                          H                            He                           n

22.   What is the term for the dissolving medium in a solution?
      a. solvent                                                c.      emulsifier
      b. solute                                                 d.      solvator

23.   What is the charge of a cation?
      a. a positive charge
      b. a negative charge
      c. no charge
      d. The charge depends on the size of the nucleus.

24.   How many electrons does barium have to give up to achieve a noble-gas electron configuration?
      a. 3                                                    c. 4
      b. 1                                                    d. 2

25.   Which of the following measurements contains two significant figures?
      a. 0.004 04 L                                           c. 0.000 44 L
      b. 0.004 40 L                                           d. 0.004 00 L

26.   What is the correct name for Sn (PO ) ?
      a. tin(II) phosphate                                         c.   tin(IV) phosphate
      b. tin(III) phosphate                                        d.   tritin diphosphate

27.   How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a phase diagram?
      a. by a line separating the phases
      b. by the planar regions between lines in the diagram
      c. by a triple point on the diagram
      d. by the endpoints of the line segment separating the phases

28.   Which of the following is the correct name for N O ?
      a. nitrogen dioxide                                          c.   nitrous oxide
      b. dinitrogen pentoxide                                      d.   nitrate oxide

29.   A skeleton equation does NOT show which of the following?
      a. the correct formulas of the reactants and products
      b. an arrow connecting the reactants to the products
      c. the reactants on the left, the products on the right
      d. the relative amounts of reactants and products

30.   Why are two nonpolar substances able to dissolve in each other?
      a. They combine to produce a polar substance.
      b. There is no attractive force between them.
      c. They have similar attractive forces in their molecules.
      d. Nonpolar substances cannot dissolve in each other.

31.   What is thought to cause the dispersion forces?
      a. attraction between ions                                   c.   differences in electronegativity
      b. motion of electrons                                       d.   sharing of electron pairs
   32.   If a sealed syringe is heated, in which direction will the syringe plunger move?
         a. out                                                        c. in
         b. The direction cannot be predicted.                         d. The plunger will not move.

   33.   A double-replacement reaction takes place when aqueous Na CO reacts with aqueous Sn(NO ) . You would expect one of the products of this
         reaction to be ____.
         a. NaNO                                                c. NaSn
         b. CNO                                                 d. Sn(CO )

   34.   Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?
         a. unshared pair                                           c. inner pair
         b. unvalenced pair                                         d. outer pair

   35.   What occurs in solvation?
         a. Ionic compounds are formed.
         b. Solvent molecules bind covalently to solute molecules.
         c. Solvent molecules surround solute ions.
         d. Solute ions separate from solvent molecules.

   36.   Which of the following statements correctly compares the relative size of an ion to its neutral atom?
         a. The radius of an anion is greater than the radius of its neutral atom.
         b. The radius of an anion is identical to the radius of its neutral atom.
         c. The radius of a cation is identical to the radius of its neutral atom.
         d. The radius of a cation is greater than the radius of its neutral atom.

   37.   What characteristic of metals makes them good electrical conductors?
         a. They have mobile protons.
         b. They have mobile cations.
         c. They have mobile valence electrons.
         d. Their crystal structures can be rearranged easily.

   38.   Which of the following is NOT true about empirical and molecular formulas?
         a. The empirical formula of a compound can be triple its molecular formula.
         b. The molecular formula of a compound can be the same as its empirical formula.
         c. The molecular formula of a compound can be some whole-number multiple of its empirical formula.
         d. Several compounds can have the same empirical formula, but have different molecular formulas.

   39.   Which of the following statements is NOT true about what happens in all chemical reactions?
         a. The ways in which atoms are joined together are changed.
         b. The bonds of the reactants are broken and new bonds of the products are formed.
         c. The starting substances are called reactants.
         d. New atoms are formed as products.

   40.   What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
         a. 3M                                                       c. 7M
         b. 6M                                                       d. 12M

41.Which symbol is used for an alpha particle?
       a.                                                             c.
            He                                                              He
       b.                                                             d.
            He                                                              He

   42.   What is the electron configuration of the calcium ion?
         a.                                                           c.
            1s 2s 2p 3s 3p 4s                                              1s 2s 2p 3s 3p
         b.                                                           d.
            1s 2s 2p 3s 3p 4s                                              1s 2s 2p 3s

   43.   What is the electron configuration of the iodide ion?
         a.
            1s 2s 2p 3s 3p 3d 4s 4p
         b.
            1s 2s 2p 3s 3p 3d 4s 4p 4d 5s
         c.
            1s 2s 2p 3s 3p 3d 4s 4p 4d 5s 5p
         d.
            1s 2s 2p 3s 3p 3d 4s 4p 4d

   44.   The reaction 2Fe 3Cl       2FeCl is an example of which type of reaction?
         a. single-replacement reaction                        c. decomposition reaction
         b. combustion reaction                                d. combination reaction
45.   Chemical equations ____.
      a. give directions for naming chemical compounds
      b. describe chemical reactions
      c. show how to write chemical formulas
      d. describe only biological changes

46.   Which of the following elements does NOT form an ion with a charge of 1 ?
      a. sodium                                             c. hydrogen
      b. fluorine                                           d. potassium

47.   Write the equation that shows the combined gas law.

48.   When the following equation is balanced, what is the coefficient for HCl?
      Mg(s) HCl(aq)       MgCl (aq) H (g)
      a. 2                                                      c. 6
      b. 1                                                      d. 3

49.   Why is hydrogen bonding only possible with hydrogen?
      a. Hydrogen is the only atom that is the same size as an oxygen atom.
      b. Hydrogen’s nucleus is electron deficient when it bonds with an electronegative atom.
      c. Hydrogen is the most electronegative element.
      d. Hydrogen tends to form covalent bonds.

50.   What is the key difference between a liquid and a gas?
      a. the ability to flow                                     c.   intermolecular attractions
      b. the motion of their particles                           d.   average kinetic energy

51.   What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the sample is increased?
      a. The change in average kinetic energy cannot be determined.
      b. The average kinetic energy decreases.
      c. The average kinetic energy increases.
      d. The average kinetic energy does not change.

52.   What is the correct formula for potassium sulfite?
      a. K SO                                                    c.   KHSO
      b. KHSO                                                    d.   K SO

53.   Chemical equations must be balanced to satisfy ____.
      a. the law of conservation of mass                         c.   Avogadro’s principle
      b. the law of definite proportions                         d.   the law of multiple proportions

54.   What is the mass in grams of 5.90 mol C H ?
      a. 0.0512 g                                                c.   673 g
      b. 389 g                                                   d.   19.4 g

55.   The equation H PO     3KOH         K PO       3H O is an example of which type of reaction?
      a. decomposition reaction                                c. double-replacement reaction
      b. single-replacement reaction                           d. combination reaction

56.   What causes hydrogen bonding?
      a. motion of electrons
      b. sharing of electron pairs
      c. attraction between ions
      d. bonding of a covalently bonded hydrogen atom with an unshared electron pair

57.   What is the number of electrons in the outermost energy level of an oxygen atom?
      a. 2                                                      c. 6
      b. 8                                                      d. 4

58.   What causes dipole interactions?
      a. attraction between ions
      b. bonding of a covalently bonded hydrogen to an unshared electron pair
      c. sharing of electron pairs
      d. attraction between polar molecules

59.   How does atomic radius change from left to right across a period in the periodic table?
      a. It first increases, then decreases.                    c. It tends to decrease.
      b. It tends to increase.                                  d. It first decreases, then increases.
60.   What is the name given to the electrons in the highest occupied energy level of an atom?
      a. orbital electrons                                       c. cations
      b. valence electrons                                       d. anions

61.   Which of the following statements is true about ions?
      a. Anions form when an atom loses protons.
      b. Cations form when an atom loses electrons.
      c. Cations form when an atom gains electrons.
      d. Anions form when an atom gains protons.

62.   A beta particle is a(n) ____.
      a. electron                                                   c.   photon
      b. helium nucleus                                             d.   hydrogen nucleus

63.   In a combustion reaction, one of the reactants is ____.
      a. oxygen                                                     c.   nitrogen
      b. a metal                                                    d.   hydrogen

64.   What does the band of stability for atomic nuclei refer to?
      a. the ratio of protons to neutrons
      b. the ratio of beta particles to neutrinos
      c. the ratio of alpha particles to beta particles
      d. the ratio of neutrons to protons

65.   Which of the following is primarily responsible for holding water molecules together in the liquid state?
      a. hydrogen bonds                                          c. polar covalent bonds
      b. ionic bonds                                             d. dispersion forces

66.   What type of ions have names ending in -ide?
      a. only metal ions                                            c.   only cations
      b. only gaseous ions                                          d.   only anions

67.   The atomic number of an element is the total number of which particles in the nucleus?
      a. protons and electrons                                c. protons
      b. neutrons                                             d. electrons

68.   What is the percent composition of carbon, in heptane, C H ?
      a. 19%                                                   c. 12%
      b. 84%                                                   d. 68%

69.   Why does a liquid's rate of evaporation increase when the liquid is heated?
      a. The surface area of the liquid is reduced.
      b. The average kinetic energy of the liquid decreases.
      c. The potential energy of the liquid increases.
      d. More molecules have enough energy to overcome the attractive forces holding them in the liquid.

70.   The fact that ice is less dense than water is related to the fact that ____.
      a. ice has a molecular structure in which water molecules are arranged randomly
      b. ice has a molecular structure that is an open framework held together by hydrogen bonds
      c. the molecules of ice are held to each other by covalent bonding
      d. the molecular structure of ice is much less orderly than that of water

71.   Which of the following compounds have the same empirical formula?
      a. CO and SO                                          c. C H and C H
      b. C H and C H                                        d. C H and C H

72.   Why do atoms share electrons in covalent bonds?
      a. to attain a noble-gas electron configuration
      b. to become more polar
      c. to increase their atomic numbers
      d. to become ions and attract each other

73.   How many valence electrons does a carbon atom have?
      a. 4                                                          c.   2
      b. 1                                                          d.   3

74.   What causes water's low vapor pressure?
      a. hydrogen bonding                                           c.   dispersion forces
      b. ionic attractions                                          d.   covalent bonding
75.   A train travels at a speed of 30 miles per hour. If 1 mile = 1.6 kilometers, how fast is the train traveling in kilometers per minute?
      a. 1.0 km/min                                                 c. 0.6 km/min
      b. 0.8 km/min                                                 d. 0.4 km/min

76.   Which atom in a water molecule has the greatest electronegativity?
      a. the oxygen atom
      b. There is no difference in the electronegativities of the atoms in a water molecule.
      c. one of the hydrogen atoms
      d. both hydrogen atoms

77.   What is the electron configuration of potassium?
      a.                                                          c.
         1s 2s 2p 3s 3p                                                 1s 2s 2p 3s 3p 4s
      b.                                                          d.
         1s 2s 2p 3s 3p 4s                                              1s 2s 3s 3p 3d

78.   If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound?
      a. 20.0%                                                c. 1.25%
      b. 55.6%                                                d. 44.4%

79.   How many covalent bonds can each carbon atom form?
      a. 2                                                        c.    3
      b. 4                                                        d.    1

80.   Which field of science studies the composition and structure of matter?
      a. chemistry                                              c. physics
      b. geology                                                d. biology

81.   What is another name for the representative elements?
      a. Group C elements                                         c.    transition elements
      b. Group A elements                                         d.    Group B elements

82.   What is the name of the alkane having five carbons?
      a. octane                                                   c.    methane
      b. pentane                                                  d.    propane

83.   What are the coefficients that will balance the skeleton equation below?
      AlCl + NaOH         Al(OH)      NaCl
      a. 1, 3, 3, 1                                               c. 1, 1, 1, 3
      b. 3, 1, 3, 1                                               d. 1, 3, 1, 3

84.   Alkanes are hydrocarbons that contain what type of bonds?
      a. at least one double bond                             c.        ionic bonds
      b. single covalent bonds only                           d.        at least one triple bond

85.   Which statement is true about electronegativity?
      a. Electronegativity generally increases from left to right across a period.
      b. Electronegativity is the ability of an anion to attract another anion.
      c. Electronegativity generally increases as you move from top to bottom within a group.
      d. Electronegativity generally is higher for metals than for nonmetals.

86.   What is the ending for the names of all binary compounds, both ionic and molecular?
      a. -ade                                                  c. -ide
      b. -ite                                                  d. -ate

87.   What is the molar mass of (NH ) CO ?
      a. 144 g                                                    c.    138 g
      b. 96 g                                                     d.    78 g

88.   The equation 2C H OH 9O               6CO      8H O is an example of which type of reaction?
      a. single-replacement reaction                             c. double-replacement reaction
      b. combustion reaction                                     d. decomposition reaction

89.   An organic compound that contains only carbon and hydrogen and at least one carbon-carbon triple bond is classified as an ____.
      a. alkane                                              c. alkene
      b. alkyne                                              d. arene

90.   How are chemical formulas of binary ionic compounds generally written?
      a. subscripts first, then ions
      b. Roman numeral first, then anion, then cation
       c.   anion on left, cation on right
       d.   cation on left, anion on right

 91.   What is the number of moles of beryllium atoms in 36 g of Be?
       a. 320 mol                                               c. 45.0 mol
       b. 4.0 mol                                               d. 0.25 mol

 92.   What symbol is used for beta radiation?
       a.                                                           c.
             e                                                            e
       b.                                                           d.
             e                                                             e

 93.   Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?
       a. 1 C and 0 kPa                                        c. 0 C and 22.4 kPa
       b. 100 C and 100 kPa                                    d. 0 C and 101 kPa

 94.   What are the coefficients that will balance the skeleton equation below?
       N +H         NH
       a. 3, 1, 2                                                  c. 1, 3, 2
       b. 1, 1, 2                                                  d. 1, 3, 3

 95.   What is the formula unit of aluminum oxide?
       a. Al O                                                      c.   AlO
       b. Al O                                                      d.   AlO

 96.   What is primarily responsible for the surface tension of water?
       a. covalent bonding                                        c. dispersion forces
       b. ionic attractions                                       d. hydrogen bonding

 97.   If a sealed syringe is plunged into cold water, in which direction will the syringe piston slide?
       a. The direction cannot be predicted.                        c. No movement will occur.
       b. out                                                       d. in

 98.   Suppose you encounter a chemical formula with H as the cation. What do you know about this compound immediately?
       a. It is an acid.                                       c. It is a base.
       b. It is a polyatomic ionic compound.                   d. It has a 1 charge.

 99.   Which of the following is NOT a characteristic of most ionic compounds?
       a. They are solids.
       b. They have low melting points.
       c. When melted, they conduct an electric current.
       d. They are composed of metallic and nonmetallic elements.

100.   Select the correct formula for sulfur hexafluoride.
       a. F S                                                       c.   F SO
       b. S F                                                       d.   SF


101.   How many moles of silver atoms are in 1.8      10     atoms of silver?
       a.                                                          c.
          3.0 10                                                         3.0 10
       b.                                                          d.
          3.3 10                                                         1.1 10

102.   The equation Mg(s) 2HCl(aq)           MgCl (aq)       H g is an example of which type of reaction?
       a. double-replacement reaction                               c. decomposition reaction
       b. combination reaction                                      d. single-replacement reaction

103.   Which of the following particles are free to drift in metals?
       a. neutrons                                                  c.   electrons
       b. cations                                                   d.   protons

104.   What causes gas pressure in a container such as a helium balloon?
       a. the vacuum maintained in the container
       b. atmospheric pressure acting on the outside walls of the container
       c. the walls of the container
       d. the simultaneous collisions of fast-moving particles in the container
 105.   What is the molar mass of AuCl3?
        a. 130 g                                                    c.   303.6 g
        b. 96 g                                                     d.   232.5 g

 106.   An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.
        a. neutral molecules                                      c. fewer electrons than protons
        b. a polyatomic anion                                     d. only two elements

 107.   Which of the following usually makes a substance dissolve faster in a solvent?
        a. decreasing the number of particles
        b. lowering the temperature
        c. agitating the solution
        d. increasing the particle size of the solute

Short Answer

 108.   The closeness of a measurement to its true value is a measure of its ____.
 109.   The direct change of a substance from a solid to a gas is called ____.
 110.   An ionic bond is a bond between ____.
 111.   Boyle's law states that ____.
 112.   The sum of the protons and neutrons in an atom equals the ____.
 113.   A compound held together by ionic bonds is called a ____.
 114.   The least penetrating form of radiation is ____.
 115.   The atomic mass of an element is the ____.
 116.   The octet rule states that, in chemical compounds, atoms tend to have ____.
 117.   When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid ____.
 118.   All atoms of the same element have the same ____.
 119.   A reaction that results in the combining of smaller atomic nuclei is ____.
 120.   In the chemical equation H O (aq)  H O(l) O (g), the               is a ____.
 121.   In every balanced chemical equation, each side of the equation has the same number of ____.
 122.   The bonds between adjacent water molecules are called ____.
 123.   The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a ____.
 124.   Binary molecular compounds are made of two ____.
 125.   The modern periodic table is arranged in order of increasing atomic ____.
 126.   When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.
 127.   When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this eaction
        is ____.
 128.   In naming a binary molecular compound, the number of atoms of each element present in the molecule is indicated by ____.
 129.   The letter "p" in the symbol 4p indicates the ____.
 130.   The simple sugars are also called ____.
 131.   An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____.
 132.   Each period in the periodic table corresponds to ____.
 133.   The lowest whole-number ratio of the elements in a compound is called the ____.
 134.   Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the
        same period tend to be ____.
 135.   As the temperature of a fixed volume of a gas increases, the pressure will ____.
 136.   The smallest particle of an element that retains the properties of that element is a(n) ____.
 137.   The names of the straight-chain alkanes all end with the suffix ____.
 138.   The particles that are found in the nucleus of an atom are ____.
 139.   The bonds between the hydrogen and oxygen atoms in a water molecule are ____.
 140.   Starch is a poly- ____.
 141.   Avogadro's number of representative particles is equal to one ____.
 142.   To what category of elements does an element belong if it is a poor conductor of electricity?
 143.   The study of chemicals that, in general, do not contain carbon is traditionally called what type of chemistry?
 144.   Charles's law states that ____.
 145.   The escape of molecules from the surface of a liquid is known as ____.
 146.   A theory is a ____.
 147.   When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____.
 148.   The charge on a gamma ray is ____.
Answer Section
MULTIPLE CHOICE
   1. D                                      30.   C                            59.   C                                88.   B
   2. D                                      31.   B                            60.   B                                89.   B
   3. B                                      32.   A                            61.   B                                90.   D
   4. A                                      33.   A                            62.   A                                91.   B
   5. D                                      34.   A                            63.   A                                92.   B
   6. A                                      35.   C                            64.   D                                93.   D
   7. C                                      36.   A                            65.   A                                94.   C
   8. B                                      37.   C                            66.   D                                95.   B
   9. A                                      38.   A                            67.   C                                96.   D
  10. A                                      39.   D                            68.   B                                97.   D
  11. A                                      40.   A                            69.   D                                98.   A
  12. C                                      41.   C                            70.   B                                99.   B
  13. B                                      42.   C                            71.   D                               100.   D
  14. A                                      43.   C                            72.   A                               101.   C
  15. B                                      44.   D                            73.   A                               102.   D
  16. D                                      45.   B                            74.   A                               103.   C
  17. D                                      46.   B                            75.   B                               104.   D
  18. C                                      47.   C                            76.   A                               105.   C
  19. C                                      48.   A                            77.   C                               106.   B
  20. A                                      49.   B                            78.   B                               107.   C
  21. C                                      50.   C                            79.   B
  22. A                                      51.   C                            80.   A
  23. A                                      52.   D                            81.   B
  24. D                                      53.   A                            82.   B
  25. C                                      54.   C                            83.   D
  26. A                                      55.   C                            84.   B
  27. A                                      56.   D                            85.   A
  28. B                                      57.   C                            86.   C
  29. D                                      58.   D                            87.   B

SHORT ANSWER


 108.   accuracy                                                        144.   the volume of a gas is directly proportional to its temperature in
 109.   sublimation                                                            kelvins
 110.   a cation and an anion                                           145.   evaporation
 111.   the volume of a gas varies inversely with pressure              146.   well-tested explanation for a broad set of observations
 112.   mass number                                                     147.   -ide
 113.   salt                                                            148.   0
 114.   alpha radiation
 115.   weighted average of the masses of the isotopes of the element
 116.   the electron configuration of a noble gas
 117.   begins to boil.
 118.   number of protons
 119.   fusion
 120.   product
 121.   atoms of each element
 122.   hydrogen bonds
 123.   single-replacement reaction
 124.   nonmetallic elements
 125.   number
 126.   -ous
 127.   2KOH BaCl            2KCl Ba(OH)
 128.   prefixes
 129.   orbital shape
 130.   monosaccharides
 131.   76 protons and 76 electrons
 132.   a principal energy level
 133.   empirical formula
 134.   higher
 135.   increase
 136.   atom
 137.   -ane
 138.   protons and neutrons
 139.   polar covalent bonds
 140.   saccharide
 141.   mole
 142.   nonmetals
 143.   inorganic

								
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