Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

AP Chemistry > Chapter 7 > Flashcards

Chapter 7 Flashcards

(105 cards)

Start Studying
1
Q

Wavelength

A

distance between two consecutive peaks or troughs in a wave

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Symbol for wavelength

A

λ

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Frequency

A

number of waves that pass a given point per second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Energy is _______ and can occur only in discrete units of size called _______

A

quantized, hv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

discrete units of size

A

hv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

quantum

A

the smallest amount of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

electrons can be viewed as a stream of “particles” called?

A

photons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

phenomenon in which electrons are emitted from the surface of a metal when light strikes it

A

photoelectric effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

when are electrons emitted from the surface of a metal?

A

when light strikes it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

when electromagnetic radiation exhibits wave properties and particulate properties is a phenomenon called?

A

dual nature of light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

diffraction

A

when light is scattered from a regular array of points or lines

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

diffraction pattern

A

bright spots and dark areas on a photographic plate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

when does a diffraction pattern occur?

A

scattered light interfere constructively to produce a bright area or destructively to produce a dark area.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

interfere constructively

A

the peaks and troughs are in phase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

interfere destructively

A

the peaks and troughs are out of phase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

continuous spectrum results when?

A

white light is passed through a prism.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

the energy of the electron is?

A

quantized

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

quantized

A

to subdivide energy into very small but measurable increments

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what is significant of the line spectrum of hydrogen?

A

indicates only certain energies are allowed for the electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is the quantum model?

A

the electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

A hydrogen atom in its lowest possible energy state is called?

A

ground state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

the electron bound to the nucleus is similar to?

A

standing wave

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

orbital

A

a specific wave function

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Heisenberg uncertainty principle

A

there is a limitation to just how precisely we know the position and momentum of a particle at any time.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Probability distribution
the probability of finding the electron at points along a line drawn outwards from the nucleus.
25
frequency symbol
v
26
why do we see visible light?
the chemical reaction that takes place within our retina
27
how does all types of electromagnetic radiation travel?
at the speed of light
28
short waves have a ____ frequency
high
29
what is wavelength measured in?
meters
30
what is frequency measured in?
Hz (hertz)
31
symbol for speed?
c
32
symbol for planck's constant?
h
33
long wavelengths have _____ frequencies.
low
34
Max Planck postulated what?
energy can be gained or lost only in whole number multiples of the quantity hz
35
a system can transfer energy only in?
whole quanta
36
Einstein proposed that electromagnetic radiation is itself?
quantized
37
electromagnetic radiation
stream of photons traveling in a wave like pattern at the speed of light.
38
photon
stream of "particles" suggested by electromagnetic radiation
39
Important conclusions of Planck and Einstein
- Energy is quantized and can occur only in quanta - Electromagnetic radiation shows characteristics of particulate matter and wave properties. (dual nature of light)
40
all matter exhibits both?
particulate and wave properties.
41
when H2 molecules absorb energy what happens to the bonds?
the bonds are broken resulting in excited atoms
42
what is produced when excess energy is released from hydrogen atoms?
An emission spectrum
43
Emission spectrum
a series of colored lines that correspond to wavelengths emitted by the glowing gas.
44
what colors does a continuous spectrum possess?
rainbow
45
Important points about the Bohr model (3)
-The model correctly fits the quantized energy levels of the hydrogen atom and only allows certain circular orbits for the electron - As the electron becomes more tightly bound, its energy becomes more negative - As the electron is brought closer to the nucleus, energy is released from the system
46
wave function
a function of the coordinates (x,y,z) of the electrons position in 3-D space
47
quantum wave mechanical model
the electron is able to move freely within its own home orbital and can gain energy and jump to a higher energy level
48
Pauli Exclusion Principle
In a given atom no two electrons can have the same set of four quantum numbers.
49
l=1
p
50
l=0
s
51
l=2
d
52
l=3
f
53
to Schrodinger and de Brigolie the electron bound to the nucleus seemed similar to?
standing wave
54
In the quantum mechanical model, Specific electron motions are?
unknown
55
In the quantum mechanical model, the specific electron motions help determine?
the most probable distance at which the electron is found
56
Principle Quantum number has ____ values?
integer
57
As n increases, what happens to the orbital and energy of the electron?
orbital becomes larger with more electrons away from nucleus. Energy is higher since electron less tightly bound to the nucleus.
58
angular momentum quantum number symbol
l
59
angular momentum quantum number has values from?
0 to n-1
60
the angular momentum quantum number is related to?
the shape of atomic orbitals
61
magnetic quantum number symbol
ml
62
the magnetic quantum number has integer values between
l and -l including zero
63
the value of ml is related to?
the orientation of the orbital in space
64
l is also called?
subshell
65
the number of nodes increases as?
n increases
66
node
area of zero probability if finding an electron
67
shape of the s orbital
spherical
68
shape of p orbitals
2 lobes separated by a node at the nucleus
69
electron spin quantum number symbol
ms
70
ms can only have two values?
+.5 and -.5
71
Since only 2 values of ms are allowed, an orbital?
can only hold two electrons and must have opposite spins
72
poly electronic atoms
atoms with more than one electron
73
3 energy contributions that must be considered of the description of poly electronic atoms?
-KE as move towards the nucleus -PE of attraction btwn the nucleus & electrons -PE of repulsion between 2 electrons
74
Electron correlation problem
since electron pathways are unknown, the electron repulsion cannot be calculated
75
electron repulsion
electrons staying as far apart from each other as possible due to their same charge
76
2s orbital is lower than a _____ orbital in poly electronic atoms
2p
77
the more effectively an orbital allows its electrons to penetrate the shielding electrons to be closer to the nuclear charge, what happens to the energy of the orbitals?
lowers
78
Aufbau principle
as protons are added one by one to the nucleus to build up elements, electrons are similarly added to the hydrogen-like orbitals
79
Hund's rule
the lowest energy for an atom is one having the max number of unpaired electrons allowed in a particular set of degenerate orbitals
80
inner elements are known as?
core elements
81
elements on which the 4f orbitals are being filled
lanthanides
82
elements on which the 5f orbitals are being filled
actinides
83
Ionization energy
energy required to remove an electron from a gaseous ion or atom in gorund state
84
In the process of ionization ______ energy electrons are removed first.
highest
85
first ionization energy
energy required to remove the highest energy electron of an atom
86
Second ionization energy
energy required to remove the highest energy electron of an ion
87
trend in ionization across a period
increase
88
why does ionization energy increase across a period?
due to increasing nuclear charge which results in electrons being more strongly bound to the nucleus
89
trend in ionization down a group
decrease
90
why does ionization decrease down a group?
due to the outermost electron being father from the nucleus
91
atomic radius
the measure of size of an element
92
trend in atomic radius across a period
decrease
93
why does atomic radius decrease across a period
due to the increase in protons the nuclear charge attracts the electrons more strongly.
94
trend in atomic radius down a group
increase
95
why does atomic radius increase down a group?
the number of energy levels increases so there is a greater distance between the nucleus and outermost orbital
96
group 1A
alkali
97
group 2A
alkaline earth metals
98
group 7A
halogens
99
group 8A
noble gases
100
metals tend to _____ electrons and form _____.
lose, cations
101
metals tend to have ______ ionization energies
low
102
where are most active metals located on the table?
bottom left corner
103
nonmetals tend to ____ electrons and form ____.
gain, anions
104
electron shielding
the blocking of valence shell electron attraction by the nucleus, due to the presence of inner-shell electrons.

AP Chemistry (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions