Ut Arlington Chem 1441 Chemistry Mcmurry Fay Chapter 5 Vocabulary

Front 1

λ is symbol for what?

Back 1

wavelength

Front 2

what is v Greek nu a symbol for?

Back 2

frequency

Front 3

what is v, frequency usually expressed in?

Back 3

1/s or s-1, or hertz

Front 4

what is MHz

Back 4

mega hertz or 1,000,000 cycles per second

Front 5

what is λ measuring?

Back 5

wavelength, one wave peak to the next peak

Front 6

Balmer-Rydberg equation

Back 6

1/λ = R(1/m2 - 1/n2)

or

v = R*c(1/m2 - 1/n2)

Front 7

What is the Rydberg constant

Back 7

1.097 x (10)-2(nm)-1

Front 8

What is the relative ordering of the various regions of the electromagnetic spectrum?

Back 8

Gamma Rays -> X Rays -> UV -> visible (VIBGYOR) -> IR -> microwaves -> radio waves

Front 9

what is the symbol for frequency?

Back 9

v, delta nu, kinda weird v

Front 10

What are two observations that did not fit with classical mechanics?

Back 10

1. Presence of a threshold frequency, v-not (Greek nu) is minimum frequency for a metal to emit an e-

2. Absence of a time lag

Front 11

Einstein proposed that a beam of light behaves as if it were composted of a string of small what?

Back 11

particles called photons

Front 12

The energy of a photon depends ONLY on what? and not what...

Back 12

energy of photon depends ONLY on frequency and NOT on intensity

Front 13

what does the intensity of light correspond to?

Back 13

the number of photons, not the energy of photons, the brighter the light the more the photons

Front 14

What's a rough analogy to explain how it's only the frequency and not the intensity that matters?

Back 14

ping pongs on a window

Front 15

in addition to performing like waves, what does light also behave like?

Back 15

particles

Front 16

Energy is quantized which means what?

Back 16

It exists only in discrete amounts

Front 17

Energy is to quanta as matter is to?

Back 17

atoms

Front 18

matter is to atoms as energy is to?

Back 18

quanta

Front 19

The light given off by excited H atoms is not a _________spectrum but rather a _________spectrum

Back 19

not a continuous spectrum but rather a line spectrum

Front 20

Esubn =

Back 20

-2.18 x (10)-18 J(Z2/n2)

where Esubn is the energy of an e- in the nth state
where Z = nuclear charge or the # of something...
where n = energy level "Bohr's orbits"

Front 21

ΔE = what conceptually

Back 21

ΔE = Esubfinal - Esubinitial

So it will always have a sign of positive or negative

Front 22

ΔE = what as a numbered equation?

Back 22

ΔE = -2.18 x (10)-18 J (1/(n-final)2 - 1/(n-initial)2)

Front 23

In this equation ΔE = -2.18 x (10)-18 J (1/(n-final)2 - 1/(n-initial)2)

Calculate the wavelength of light emitted or absorbed when a H e- goes from n= 2 to n=4

Back 23

ΔE = -2.18 x (10)-18 J (1/(4)2 - 1/(2)2)

ΔE = -2.18 x (10)-18 J (1/(4)2 - 1/(2)2)

Front 24

If ΔE is positive, then it's emitting or absorbing?

Back 24

It's absorbing

Front 25

If ΔE is negative, then it's emitting or absorbing?

Back 25

emitting

Front 26

What is the wavelength range of visible light?

Back 26

400-750 nm

Front 27

Quantum mech says that the amt of energy that can be transferred is what?

Back 27

quantized; that is, energy can only be transferred in discrete units of size called: hv (v=Greek nu)

Front 28

Energy is what?

Back 28

Energy is quantized

Front 29

the smallest "packet" of energy is called what

Back 29

quantum

Front 30

an individual packet or particle of electromagnetic radiation is called a what?

Back 30

photon

Front 31

Up to this point, science was indicating that light which is _____ has ______ characteristics.

Back 31

Up to this point, science was indicating that light which is _wavelike_ has _particle-like__characteristics.

Front 32

de Broglie proposed that if energy is _____ then perhaps matter is ________ .

Back 32

de Broglie proposed that if energy is _particle-like_ then perhaps matter is _wavelike__ .

Front 33

λ = what formulaicly

Back 33

h/mc

Front 34

Niels Bohr initially suggested that electrons exist in what?

Back 34

orbits

Front 35

QM treats electrons differently, QM says an e- has both what and what properties?

Back 35

particle-like and wave-like

Front 36

The Heisenberg uncertainty principle says it is impossible to know both the ___ and the ____ of a particle simultaneously

Back 36

position and momentum

Front 37

what is h in Ephoton = hv?

Back 37

h is Planck's constant which is 6.626 x 10 -34 J*s

Front 38

what is de Broglie's eqn?

Back 38

λ = h/(m*v) where v is Greek mu

Front 39

What is the Rydberg constant?

Back 39

-2.18 x (10)-18

Front 40

What's the formula to calculate change in energy? (One state to the next?)

Back 40

1/λ = R(1/m2 - 1/n2) where m is the smaller number and n is the bigger number

Front 41

Instead of assigning ______ ______ for electrons, the most we can hope to know is the _______ of finding an e- in a given region of space

Back 41

fixed paths; probability

Front 42

since an e- has wave-like properties, quantum mechanics is also called ____ _____

Back 42

wave mechanics

Front 43

QM is a ____ _____ description of an e-

Back 43

mathematical description

Front 44

When Schrodinger's eqn is solved for the lowest energy e- in hydrogen, you get 1. _____ & 2. ______

Back 44

1. Quantum numbers
2. Electron config's

Front 45

how can you measure the intensity of a wave?

Back 45

amplitude

Front 46

what is amplitude of a wave?

Back 46

height

Front 47

what is the principle quantum number?

Back 47

n, describes the "shell" of the e-, possible values are n=1,2,3,etc

Front 48

what is the angular momentum quantum number?

Back 48

l, describes the shape of the orbital
l=0 -> s
l=1 -> p
l=2 -> d
l=3 -> f

Front 49

l=0 corresponds to what shape?

Back 49

s - sphere

Front 50

l=1 corresponds to what letter?

Back 50

p, hourglass

Front 51

l=2 corresponds to what letter?

(and looks like what...)

Back 51

d, kind of clover looking thing and the half clover with doughnut ring

Front 52

l=3 corresponds to what letter?

Back 52

f

Front 53

what is the magnetic q.n.?

Back 53

(m)sub-l, describes orientation in space of the orbital

expressed as (m)sub-l= -l....0....+l

Front 54

what is the spin q.n.?

Back 54

(m)sub-s, describes the spin of e-, expressed as +1/2 or -1/2

Front 55

how do you show upspin?

Back 55

+1/2

Front 56

how do you show down-spin?

Back 56

-1/2

Front 57

what is aufbau?

Back 57

start in low energy orbitals and build up

Front 58

what is Pauli exclusion principle

Back 58

there can be a max of 2 e- per orbital as long as they have opposite spin (up and down half arrows)

No 2 e- in an atom can have the same 4 q.n.'s

Front 59

Hund's rule

Back 59

(parallel before paired)

when filling degenerate orbitals e- occupy them singly one at a time. with parallel spin before pairing up

Front 60

ground state

Back 60

lowest energy state

Front 61

excited state

Back 61

not the ground state...any other state of the atom

Front 62

degenerate

Back 62

equal in energy, for example the 3 2p orbitals are equal in energy or "degenerate"

Front 63

node

Back 63

a region in space with zero probability of finding an e-

Front 64

shell

Back 64

n, for example n=4 shell

Front 65

subshell

Back 65

(n)sub-l, for example 4s subshell, 4p subshell

Front 66

where are the s, p, d, f blocks?

Back 66

s is col 1&2
p is col 13-18
d is col 3-12
f is inner transition metals

Front 67

There is a special stability associated with ________

Back 67

filled outermost subshells, for example the noble gasses

Front 68

There is another special stability associated with _____

Back 68

exactly half-filled outermost subshells for ex. the 3- config of Cu & Cr, 1st IE of N&O

Front 69

When determining the e- config of cations, the first electrons removed are ____

Back 69

the from the outermost shell, not necessarily the outermost subshell (watch T.M cations)

Front 70

isoelectric

Back 70

have exactly the same e- config; same energy

Front 71

paramagnetic

Back 71

attracted into a magnetic field (Has one or more unpaired e- (Imagine the slates __ __ __ and they've only got an upward pointing electron in at least one of them.

Front 72

diamagnetic

Back 72

slightly repelled by a magnetic field *ALL e- are paired (Imagine the blank slates __ __ both have an up and a downward pointing e- filling them.)

Front 73

valence electrons

Back 73

outer shell e-'s

Front 74

core electrons

Back 74

inner shell e-'s

Front 75

write the complete ground state e- config for:

F

Back 75

1s2 2s2 2p5

Front 76

write the complete ground state e- config for:

F-

Back 76

1s2 2s2 2p6

Front 77

write the complete ground state e- config for:

Ne

Back 77

1s2 2s2 2p6

Front 78

write the complete ground state e- config for:

Na

Back 78

1s2 2s2 2p6 3s1

Front 79

write the complete ground state e- config for:

Na+

Back 79

1s2 2s2 2p6

Front 80

What are the exceptions to the e- config rules?

Back 80

Cr - [Ar]4s1 3d5
paramagnetic w/ 6 unpaired e-

Cu - [Ar]4s1 3d10
paramagnetic w/ 1 unpaired e-

Cr Cu
Mo Ag
*Not*W* Au

Front 81

shielding

Back 81

screening; the ability of other e- especially inner core e-'s to decrease the nuclear attraction for an out e-

Front 82

effective nuclear charge

Back 82

(Z)sub-effective - the nuclear charge that the e- actually "feels" or experiences as a result of the shielding of other e-'s

Front 83

To predict periodic trends, consider 2 things:

Back 83

1. e- config
2. nuclear charge, Z, # protons

Front 84

As you go down the periodic table what happens to size?

Back 84

It goes up

Front 85

As you go across the periodic table what happens to size

Back 85

It goes down

Front 86

As you go left on the periodic table what happens to size

Back 86

It goes up

Front 87

as you go up on the periodic table what happens to size

Back 87

It goes down

Front 88

Atomic size _____ going from left to right across the periodic table because: ____

Back 88

decreases; because of increasing nuclear charge. There's more positive protons (Z) in the nucleus pulling them in tighter on the right side, and fewer positive protons Z on the left side

Front 89

Atomic size ____ going down the periodic table because _____

Back 89

increases; because e- are going into the higher shells
--Also because the inner core e- are shielding outer core e- from the nuclear charge

Front 90

Which is bigger? Cation or parent atom?

Back 90

Parent atom is always bigger than its cation

Front 91

Which is bigger? anion or parent atom?

Back 91

Anion is always bigger than its parent atom

Front 92

In isoelectronic cases, how do you decide which is isoelectronic?

Back 92

Has same exact e- configuration

Front 93

What (m)sub-s?

Back 93

spin quantum number;

measures spin of the e-

Expressed as either +1/2 or -1/2

Front 94

definition of ionization energy

Back 94

Energy required to remove an e- from a gaseous atom or ion

Front 95

General trends of IE?

Back 95

Up going up on periodic table
Up going --> on periodic table

**BUT important exceptions

Ei1 = 1st IE (ionization energy); energy req'd to remove the first e-

Ei2 = 2nd IE ....""""...."" second e-

Ei3 = 3rd IE ....."" to remove third e-

Ei4 = etc
etc

Front 96

Which is greater, Ei1(Na) or Ei2(Mg)?

Back 96

Ei1(Mg) because we're removing a 3s e- in both cases but Mg has a greater nuclear charge Z

Front 97

Place following in order of increasing Ei1:

Li Be B C N O F

Back 97

Li < B < Be < C < O < N < F

Front 98

Electron affinity definition

Back 98

energy change that occurs when an e- is added to a gaseous atom

Front 99

Some electron affinities are ___ and some are ____

Back 99

some positive and some negative

Front 100

If the electron affinity is negative, that means what?

Back 100

the atom "wants" and e-

ΔE = Efinal - Einitial
The more negative the EA, the more the atom "wants" the e-

Front 101

Groups ___ and ____ has positive (endothermic) electron affinities:

Back 101

Groups 2 & 18 -

Alkaline Earth metals
Noble gasses

Front 102

The _____ have the most exothermic - negative electron affinities

Back 102

halogens - col 17

Front 103

How do we make individual predictions about EA's?

Back 103

1. Electron config
2. nuclear charge

Front 104

The 3 types of chemical bonding are:

Back 104

1. Ionic bonding
2. Covalent bonding
3. Metallic bonding

Front 105

1. Ionic bonding

Back 105

electrostatic attractions between oppositely charged particles

Front 106

2. Covalent bonding

Back 106

atoms share valence e-

Front 107

3. Metallic bonding

Back 107

metal cations sitting in a "sea" of e-

Front 108

octet rule

Back 108

atoms tend to gain, lose or share e- in such a way as to attain a noble gas e- config

Front 109

When considering Ionic and Covalent bonding as a continuum, discuss:

Ionic bonding

Back 109

- involves complete e- xfer
- exists in an infinite 3D crystal lattice
- solids at room temp with very high mp's

Front 110

When considering Ionic and Covalent bonding as a continuum, discuss:

Polar Covalent

Back 110

- unequal sharing of e- (Ex HCl the cloud leans more toward Cl)
...this makes the HCl have a slightly + on the H side and slightly - on the Cl side
- This sharing could be written:
H - Cl
+----->

Front 111

When considering Ionic and Covalent bonding as a continuum, discuss:

Nonpolar Covalent

Back 111

- involves equal sharing of e-
- individual molecules (As compared to infinite crystal lattices)
- usually gasses or liquids at room temp or at least very low MP solids (MP < 200 C)

Front 112

What is the key concept to understanding and classifying comp between 2 atoms?

Back 112

Electronegativity

Front 113

3 things to consider in terms of energy with respect to ionic bonding and lattice energy

Back 113

1. Metals have low IE
2. NM have high EA
3. Energy is released when gaseous ions form solid crystal

Front 114

lattice energy

Back 114

the energy req'd to separate 1 mole of a solid ionic crystal into gaseous ions far removed from each other

Front 115

How does Lattice Energy relate to some of the physical properties of ionic substances?

Back 115

In general the higher the lattice energy:
1. The higher the MP
2. The harder the substance

Front 116

Bond breaking is always ___thermic

Back 116

endothermic

Front 117

Bond formation is always ____thermic

Back 117

exothermic

Front 118

Coulomb's law

Back 118

F= k*[(Qsub1Qsub2)/d2]

where F = force of attraction or repulsion between two charged particles
Q1, Q2 = magnitudes of charges
d= distance between 2 centers

Front 119

Coulomb's law says generally the ____ the ionic charge the ____ the lattice energy

Back 119

greater greater

Front 120

Coulomb's law says generally the ____ the ion charge the ____ the lattice energy

Back 120

smaller greater

Front 121

Which is more important, charge or size when applying Coulomb's law to lattice energy?

Back 121

CHARGE usually more important than SIZE

Front 122

Arrange following ionic compounds in order of increasing lattice energy:

NaF, CsI, CaO

Back 122

CsI < NaF < CaO

Front 123

Which compound has the greatest lattice energy?

AgCl CuO CrN

Back 123

CrN

Front 124

Covalent bond is formed when?

Back 124

when atoms share e-

Front 125

covalent bonds are typically seen between ____

Back 125

two nonmetal elements

Front 126

Two measures of strength of a bond

Back 126

1. bond length
2. bond dissociation energy --> covalent bond like H (this is a number like on that charge of + and - numbers)

Front 127

The _____ the bond, the ____ the bond

Back 127

shorter stronger

Front 128

Is bond breaking endo or exo?

Back 128

always endothermic (takes energy)

Front 129

is bond formation endo or exo?

Back 129

bond formation is always exothermic (gives off heat)

Front 130

mnemonic for remembering whether exo or endo on bond breaking and forming?

Back 130

a couple coming together creates heat
a couple coming apart grows cold and saps energy