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Chem 11 Chapter 10 Name ________________
Electrons in Atoms Block ___
The modern picture of the atom does not concern itself so much about the location of the electron, but
rather the ___________ level of the electron. To fully understand the model of the atom, it is necessary
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to understand how _____________ work. The fixed amount of energy changes an electron undergoes
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means electrons are said to be _______________. 3
The view of the atom changed from
______________ ’s solid sphere atom, to _____________________ proton/electron view then to
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Rutherford’s view of a central ____________ which is positively charged and orbiting at high speed the
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_______________. Missing from Rutherford’s model was the fact, according to his model, that the
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atom should be __________, but however it was not - giving rise the need to revise the model.
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In order to fully understand energy it is needed to understand the motion of ____________. When 9
viewing waves you can measure different parts of the waves. The number of times a wave passes a point
in a given period of time is known as _______________. To measure these occurrences the Greek letter
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nu _______ is used. Another property of waves is distance between to corresponding parts of the wave,
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known as ____________. The Greek letter __________ symbolized as _____ is used to identify the
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wavelength. Lastly the height of the waves is known as ________________. When viewing waves on 15
the ocean, it becomes evident that the waves do not carry the water, but rather
___________________________________________. 16
Waves do not only travel on water, but we hear
_________ waves and we can think of what we see (_________ waves) as traveling in waves. The
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different colours of light from the rainbow is known as the continuous ______________ 19
and
corresponds to light of particular range of ______________ and _______________. 20 21
In 1900 German scientist _____________________ discovered that glowing solids had emissions that
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varied with temperature. He realized that as the colour changed (wavelength) , so did the ___________ 23
of the _________. Energy values varied by small ___________ numbers. The conclusion was that
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small packets of energy was involved, an idea proposed later by ____________________ The small 26
packet of light became known as _______________. Each frequency of light has its own specific
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energy and no other – light is therefore said to be _____________. So light can be thought of as both 28
______________ and _______________. When waves are standing, the point at which the amplitude
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is zero is known as the _____________. Important is the fact this point can be located in this fraction of
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the waves ________ and not other fractions. So standing waves have discreet points or increments.
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Another important point is the fact that when the waves increase in frequency, they will decrease in
_______________. 33
1 Chem11 04 Chapter 10 Atom Electron Worksheet.doc
The light we are familiar with is produced by a combination of electrical and ______________ fields 34
(known as _________________ waves) . Waves of light (and other forms) vary in their frequency from
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________ - waves ( ? = 104 Hz) to __________ rays ( ? = 10 24 Hz ). If the wavelength and frequency
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of light is compared, as the frequency increases then the wavelength will _____________, but always 38
the product between the two is ______________________________. 39
As the energy of a wave
increases, the _____________ will also increase (consider moving a spring faster and faster to produce
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more waves – see figure 10-5 page 282). One very useful form of electromagnetic waves is
_____________ - used in dentistry, medicine, analytical chemistry, etc. The wavelength of these rays is
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about the diameter of an __________. (mmmm very interesting!! )
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The simplest of all atoms is ________________, so it is used to illustrate the relationship between
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waves and atoms. When looking at the light given off by gas tubes, an interesting phenomenon can be
seen. The light is not a complete colour spectrum, but rather a series of discreet colours only – known as
the ___________________ spectrum. The spectrum of each element is _____________ . Under low
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pressure, hydrogen will emit only _________ colours of light. The sequence of lines was following a
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mathematical progression discovered by Swiss schoolteacher _____________ . Neils Bohr explained 47
the hydrogen spectrum was due to the fact that ___________ was absorbed, while light of a certain
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_____________ was being given off. The atoms absorb energy and exist in a higher __________
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level. These atoms that have absorbed energy are referred to as being in an ___________ state. The 51
specific colour of light given off is related to the excited atom returning to its ____________ state. The 52
different levels an electron can be found, can be compared to a cat on ____________ - the higher up 53
the greater the energy level. And of course, the cat can not be part way up the stairs, only on a particular
________, 54
so the energy level of the cat is in discreet stages. In the atom, the greater the
____________-____________ distance the greater the potential energy. Validating Bohr’s theory was
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the prediction of spectral lines in the _______________ 56
and _____________ 57
regions of the
electromagnetic spectrum.
Summarize Bohr’s conclusions of the hydrogen spectrum;
58. _________________________________________________________________________________________
59. _________________________________________________________________________________________
60. _________________________________________________________________________________________
_________________________________________________________________________________________
61. _________________________________________________________________________________________
_________________________________________________________________________________________
_________________________________________________________________________________________
The “staircase” of energy levels for hydrogen are not evenly _____________ and represent the amount
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of energy per ____________ that is given off when the atom changes from a higher level. The lines of
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2 Chem11 04 Chapter 10 Atom Electron Worksheet.doc
colour from the bright-line spectrum are known as the ___________ series. The energy difference
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between higher and higher energy levels becomes ____________. So an energy from any level to level
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one will yield the greatest energy change and releases energy in ______________ region of the 66
electromagnetic spectrum. A very important amount of energy for hydrogen is ________ kJ , which 67
represents the amount energy of one mole of hydrogen to completely removed its electron – called
_________________ energy. This amount of energy for any element is the amount of energy needed to
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remove an electron from the ______________ state. Bohr’s planetary view of the electron worked well
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for ____________ but when applied to other elements the theory fell short. A new theory was needed
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and this led scientists to believe rather than a path for the electron, the ________________ or 71
likelihood of the position of the electron. The probable location or ____________ is the region in space
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an electron is most likely to be found. The lowest energy state is often called the __________ state. The 73
probability the electron will found in this orbital ranges from ____________ percent. Think of this
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probability as students in class. Students are supposed to be in class in between bells, but there is a small
chance students are in the hall or washroom (or on the boulevard smoking!!!) . Another view is the holes
found in a ____________ , where closer to the center the more holes are likely to be found. When and
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where the holes were formed is not certain, but gives an idea of the likelihood of their position. The
electron found in the ground state is located in the first energy level n=1, second energy level n=2 and so
on called the principal _________________. The specific number of orbitals possible is related to the
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____________ of its quantum number. There is only one orbital for the first energy level – called the
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____ orbital. If an electron absorbs enough energy to be in level two, it may occupy any one of _____
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orbitals. One of the orbitals in the second level is spherical 2s orbital, but three are double-_________ 80
shaped; called the 2p orbitals and is oriented in three dimensions - labeled _____, _____, and _____. 81
The nodes of the three orbitals is a place where the probability of finding the electron is _________. In 82
level three there will be a total of ________ orbitals. In the third level there are the 3s, 3p x, 3py, 3pz and
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then _____ more levels; designated the ____ orbital. At the fourth level there a total of ____ orbitals;
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the s, p, d and f orbitals, often called ____________. Each orbital has exactly the ________ energy.
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Losing energy from the fourth orbital results in the same ______-______ light in the visible spectrum.
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There are four ways to describe a particular orbital n, l, m and ms where ;
“n” is the __________ 90
and range from __________________________________________ 91
“l” is the __________ of the orbital and the letters used are __________________________
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“m” is the __________ 94
and for the 2nd level are designated ___________________________ 95
“ms ” is the __________ and can be denoted (see page 295) ________________________________
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3 Chem11 04 Chapter 10 Atom Electron Worksheet.doc
