Lect 3 supp by 2U3cbl0

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									2.9 Use the helium-4 isotope to define atomic number and mass
number. Why does a knowledge of atomic number enable us to deduce
the number of electrons present in an atom?



2.10 Why do all atoms of an element have the same atomic number,
although they may have different mass numbers?



2.11 What do we call atoms of the same elements with different mass
numbers?

Problems
2.13 What is the mass number of an iron atom that has 28 neutrons?




2.14 Calculate the number of neutrons of 239Pu.




2.15 For each of the following species, determine the number of
protons and the number of neutrons in the nucleus:
      3
        2He,

      4
          2He,

     24
       12Mg,
      25
        12Mg,

      48
        22Ti,

      79
        35Br,

      195
         78Pt




2.16 Indicate the number of protons, neutrons, and electrons in each of
the following species:
15
  7N,

33
  16S,

63
  29Cu,

84
  38Sr,

130
   56Ba,

186
   74W,

202
   80Hg




2.17 Write the appropriate symbol for each of the following isotopes:
(a) Z = 11, A = 23;

(b) Z = 28, A = 64.
2.18 Write the appropriate symbol for each of the following isotopes:
(a) Z= 74, A = 186;


(b) Z = 80, A = 201.

2.19 What is the periodic table, and what is its significance in the study
of chemistry?



2.20 State two differences between a metal and a nonmetal.


2.21 Write the names and symbols for four elements in each of the
following categories:
(a) nonmetal,

(b) metal,

(c) metalloid.


2.22 Define, with two examples, the following terms:
(a) alkali metals,
(b) alkaline earth metals,
(c) halogens,
(d) noble gases.


Problems
2.23 Elements whose names end with ium are usually metals; sodium is
one example. Identify a nonmetal whose name also ends with ium.


2.24 Describe the changes in properties (from metals to nonmetals or
from nonmetals to metals) as we move
(a) down a periodic group and
(b) across the periodic table from left to right.


2.26 Group the following elements in pairs that you would expect to
show similar chemical properties:
K
F
P
Na
Cl
N


2.27 What is the difference between an atom and a molecule?


2.28 What are allotropes? Give an example. How are allotropes
different from isotopes?
2.30 Give an example of each of the following: (a) a monatomic cation,
(b) a monatomic anion, (c) a polyatomic cation, (d) a polyatomic anion.




2.31 Which of the following diagrams represent diatomic molecules,
polyatomic molecules, molecules that are
not compounds, molecules that are compounds, or an elemental form
of the substance?




2.32 Which of the following diagrams represent diatomic molecules,
polyatomic molecules, molecules that are not compounds, molecules
that are compounds, or an elemental form of the substance?
2.33 Identify the following as elements or compounds:
NH3
N2
S8
NO
CO
CO2
H2
SO2

2.34 Give two examples of each of the following:
(a) a diatomic molecule containing atoms of the same element,

(b) a diatomic molecule containing atoms of different elements,

(c) polyatomic molecule containing atoms of the same element,

(d) a polyatomic molecule containing atoms of different elements.



2.35 Give the number of protons and electrons in each of the following
common ions:
Na+

Ca2+

Al3+

Fe2+

I-
F-

S2-

O2-

N3-.

2.36 Give the number of protons and electrons in each of the following
common ions:

K+

Mg2+

Fe3+

Br-

Mn2+

C4-

Cu2+.

								
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