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Chemistry 111 > Test 3 Study Guide > Flashcards

Test 3 Study Guide Flashcards

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1
Q

What is wavelength?

A

the distance between one peak and the next

*the measurement of wavelength is between peak to peak or trough to trough

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2
Q

As wavelength increases, the frequency?

A

decreases

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3
Q

What is the speed of light?

A

c=wavelengthXfrequency=300x10^8 m/s

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4
Q

What is the unit of frequency?

A

per second

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5
Q

1 hertz=

A

1 sec^-1

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6
Q

100.3 MHz=

A

wavelength

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7
Q

What is the principle quantum number?

A

N

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8
Q

What symbol is the angular momentum quantum number?

A

L (cursive)

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9
Q

What is the symbol for the magnetic quantum number?

A

M sub e

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10
Q

What is the symbol for the spin quantum number?

A

M sub s

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11
Q

What does the principle quantum number tell us?

A

energy or distance from nucleus

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12
Q

What numbers is the principle quantum number (n) allowed to be?

A

1,2,3,4

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13
Q

And N (principle quantum number) increases, what does E do?

A

increase

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14
Q

What does L (angular momentum quantum number decribe?

A

Tells the shape

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15
Q

What is the angular momentum quantum number allowed to be?

A

n-1 but 0 is the least it can be

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16
Q

If you know n and L, then what are you describing?

A

a subshell

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17
Q 
What letters go along with L for the various subshells?
0
1
2
3
A

0-s
1-p
2-d
3-f

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18
Q

What is the highest subshell?

A

f or 3

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19
Q

Give the protocol for naming a subshell

A

use value->nl

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20
Q

What does the magnetic quantum number tell?

A

Orientation in 3D space

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21
Q

If we know n, L, and M sub l we are describing?

A

an atomic orbital

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22
Q

Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
a) n=4, L=1, m sub L=0

A

a)allowed 4p

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23
Q

Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
b) n=2, L=2, m sub L = -1

A

Not allowed, because n & l cannot be equal

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24
Q

Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
n=5, L=3, m sub L= +3

A

Allowed, 5f

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25
Q

What does the spin quantum number tell us?

A

about magnetic properties

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26
Q

What is # are allowed in the spin quantum number?

A

+1/2

-1/2

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27
Q

If we know n, L, m sub L, and m sub s, then we are describing?

A

an individual electron

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28
Q

The s orbital makes what shape?

A

spherical

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29
Q

The p orbital makes what shape?

A

a infinity symbol

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30
Q

The d orbital makes what shape?

A

a flower w/4 petals shape

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31
Q

The f orbital makes what shape?

A

a flower with many petals

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32
Q

Nature looks for?

A

the lowest energy arrangement possible

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33
Q

What is effective nuclear charge?

A

weighted average of nuclear charge that affects an electron in the atom, after correction for the shielding by inner electrons and interelectronic repulsions

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34
Q

The _________ the affected nuclear charge, the more able the nucleus is able to control the electrons and vice versa

A

the greater the affected nuclear charge

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35
Q

Give the order of the subshells-

A

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<5d<6p etc.

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36
Q

What is the Pauli exclusion principle?

A

No two electrons in the same atom can have the same set of four quantum numbers

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37
Q

What is the Aufbau Principle?

A

as electrons are added to an atom one at a time they are assigned the quantum numbers of the lowest energy orbital that is available

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38
Q

The ground state is?

A

the lowest energy state possinle

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39
Q

What is hund’s rule?

A

One electron occupies earch degenerate orbital with the same spin before a second electron is placed in an orbital

40
Q

Group 1A atoms always form?

A

1+ cations

41
Q

Which group of atoms is particularly stable?

A

Noble gases

42
Q

What are valence electrons?

A

those with the highest principle quantum number and any electrons in a unfilled subshell from a lower shell

43
Q

What is an ion?

A

charged particle

44
Q

A cation is

A

forms a positive charge from loosing an electron

45
Q

An anion is

A

negative charge from an atom gaining an electron

46
Q

What is an isoelectronic series?

A

is a group of atoms and ions that contain the same number of electrons

47
Q

What is an example of an isoelectronic series?

A

S2-, Cl-, Ar, K+, and Ca2+

48
Q

How is the size of an atom determined?

A

by measuring its radius

49
Q

What type of atom has the smallest size?

A

Species with the highest number of protons

50
Q

Atoms are always larger than their _______.

A

Atoms are always larger than their cations

51
Q

Atoms are always smaller than their _______.

A

Atoms are always larger than their anions.

52
Q

Effective nuclear charge increases?

A

up and to the right

53
Q

As zeff increases, size?

A

decreases

54
Q

Atomic radi increase?

A

down and to the left of the periodic table

55
Q

What is ionization energy?

A

the energy required to remove an electron

56
Q

1st ionization Energy increases?

A

1st ionization Energy increases to the right and from the bottom to top

57
Q

What are the exceptions to 1st ionization energies?

A

Group IIIA and VIA exceptions

58
Q

An isoelectronic species with the greatest charge in the nucleus will have?

A

the largest ionization energy

59
Q

Successive Ionizations are always?

A

larger than 1st ionization energies

60
Q

What produces a much larger ionization energy?

A

when a non-valence electron is removed

61
Q

What is Electron affinity?

A

energy change when a electron is added to an atom to a gaseous atom to form an anion

62
Q

What is the equation for electron affinity?

A

A(g) + e- ->A-(g)

63
Q

The reactivity of the Group 1A metals increases?

A

The reactivity of the Group 1A metals increases down the group

64
Q

What are alloys?

A

mixture of metals

65
Q

The halogens all exist as?

A

diatomics

66
Q

Halogen reactivity increases as you go?

A

up the group

67
Q

What is ionic bonding?

A

+/- attracted to form bonds

68
Q

What is covalent bonding?

A

The sharing of electrons

69
Q

What is lattice energy?

A

the energy required to seperate one mole of ionic solid into its gaseous ions

70
Q

As charge goes up, lattice energy goes?

A

up

71
Q 
*************
as r (distance between ions) goes up, then lattice energy goes?
A

down

72
Q

To arrange by increasing lattice energy you?

A

assess charge first and then distance

73
Q

Ionic bonding is?

A

a metal and a nonmetal cations and anions electron transfer

74
Q

What is bond order?

A

the number of electron pairs shared between two atoms

75
Q

What is the bond order below?

a) N-N
b) N=N

A

a) 1

b) 2

76
Q

As bond order increases, bond length?

A

decreases

77
Q

As bond order increases, bond strength?

A

increases

78
Q

What are the steps to writing Lewis Dot structure

A

1) Skeleton structure
2) Sum valence electrons
3) Subtract 2e- for every bond in skeleton structure
4) Count electrons needed to complete (need) structure
5) Add extra electron as base pai

79
Q

If the electron sharing is equal, what type of bond is it?

A

a nonpolar convalent bonding

80
Q

If electron sharing is not equal, what type of bond is it?

A

polar covalent bonding

81
Q

What is electronegativity?

A

a measure of the ability of an atom to attract the shared electrons in a chemical bond

82
Q

Electronegativity increases?

A

up and to the right

83
Q

As the difference in electronegativity increases, the polarity of the bond?

A

increases

84
Q

The most polar bond will have?

A

the biggest difference in electronegativity

85
Q

The central atom is?

A

the least electronegative element

86
Q

How do you calculate formal charge?

A

The # of valence electrons - # of bonds - # of lone electrons = formal charge

87
Q

What Lewis structures are favored?

A

the structures of the smallest formal charge

88
Q

What are the rules for evaluating the stability of structures?

A

Smallest formal charge favored
Structures with adjacent atoms with formal charges of the same sign are much less favored
Lewis structures that place negative formal charges on more electronegative atoms are favored
Formal charges of opposite signs are usually on adjacent atoms

89
Q

What is a resonance structure?

A

when a molecule has more than 1 formal charge

90
Q

No resonance structure is correct by itself, how is the correct structure formed?

A

By the average between all the resonance structures

91
Q

What molecules disobey the octet rule?

A 
H needs 2e- to be stable
He needs 2e- to be stable 
2A&amp;3A central atoms don't need all electrons 
Group IIA central atoms need 4e-
Group IIIA central atoms ned 6e-
Expanded valence shell z>15
92
Q

____ formal charge is more favored than ___ formal charge.

A

No formal charge is more favored than any formal charge.

93
Q

An expanded valence shell molecules have?

A

more than eight electrons about an atom in a Lewis structure

94
Q

bond energy is?

A

the energy required to break bond

95
Q

Bond energies are always?

A

endothermic because it takes energy to break a bond

Chemistry 111 (2 decks)

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