Chapter 2 review Flashcards
1
Q
what is the quantum mechanical model?
A
explains how electrons exist and behave in atoms
2
Q
what is electromagnetic radiation?
A
light that travels by waves
3
Q
what is wavelength
A
measure of the distance covered by a wave
4
Q
what is amplitude?
A
the height of the wave
5
Q
what is the symbol for wavelength
A
lambda
6
Q
what is color?
A
when all the wavelengths of light are not absorbed
7
Q
what is frequency?
A
number of waves passing a given point per unit of time is the frequency
8
Q
what relationship does frequency and wavelength have?
A
frequency and wavelength have an inverse relationship
9
Q
what is total energy proportional to?
A
the amplitude and frequency of the waves
10
Q
if there is a large amplitude what happens to the force?
A
the force increases
11
Q
what is the speed of light(c)
A
constant speed that all electromagnetic waves move through
12
Q
what is the equation for c=
A
c = (wavelength)(frequency)
13
Q
what does c equal
A
3.00 x10^8
14
Q
what is the electromagnetic spectrum?
A
all wavelengths of electromagnetic radiation
15
Q
what are the colors of the spectrum
A
ROYGBV and it is in increasing order of frequency / decreasing length of wave
16
Q
who was max planck?
A
discovered that energy of matter was not continuous
17
Q
what is quanta?
A
discrete packets of light
18
Q
what is quantized energy?
A
energy that can be lost or gained
19
Q
what is the equation for quantized energy?
A
E = nhv
20
Q
what does h equal (planck’s constant)
A
6.626x10-34
21
Q
what did albert einstein do?
A
proposed that radiation was quantized by particles called photons
22
Q
what are the 2 equations for photons?
A
Ephoton = Hv
E photon = Hc/ wavelength
23
Q
what does a short wavelength mean?
A
high frequency and high energy
24
Q
what is threshold frequency?
A
the minimum frequency required before electrons would emit intensity
25
what is the KEelectron equation
1/2mv^2=hv-hV0
26
what did louis de brogile theorized
if light can have material properties matter should exhibit wave properties
-predicted that the wavelength of inversely proportional to its momentum
27
what does wavelength =
lambda = h/mv
28
what is interference
the interacton between waves
29
what is constructive interference
when waves interact so that they add to make a larger wave
30
what is destructive interference?
when waves interact so they cancel each other it is
31
what is diffraction?
when traveling waves encounter an obstacle or opening in a barrier that is about the same size as the wavelength an they bend around it
32
what are complimentary properties?
only one aspect of wave or particle can be obserbed
| both can never be observed at the same time
33
what is a spectrum?
common radiation source that contains many different wavelength components
34
what is a continuous spectrum?
when light is produced through a prism
35
what is a line spectrum
discrete wavelengths is observed
36
what is atomic emission?
different gases emit light of different characterisitc colors upon excitation by electrical discharge
37
what is a flame test?
used to identify the presence of certain elements, primarily group 1 metal ions
38
who created the bohr model
niels bohr
39
what does the bohr model explain
where the electrons are and how the atom changes when it undergoes energy transitions
40
what are stationary states?
electrons travel in orbits that are fixed distance from the nucleus
41
what happens when attraction goes up?
the energies are more negative
42
what happens when n goes up
attraction goes down
43
how do we calculate the energy level of n
En = -2.18x10^-18J (1/n^2)
44
what is the formula to find the change in electron?
change in energy level = -2.18x10^-18J(1/nf)^2-(1/(ni)^2
45
what is the uncertainty principle?
heisenburg stated that the product of the uncertainties in both the position and speed was inversely proportional to its mass
46
what is the change in mass and velocity
uncertainty in momentum
47
what is the change in x
uncertainty in position
48
what is classical physics?
a particles velocity , positon, and forces acting on it are known
49
what is quantum mechanics?
a particles position or its velocity can be known but not both
50
is classical physics determinacy or interminacy?
determinacy
51
what is determinacy?
definite or a predictable future
52
indeterminacy?
indefinite future
53
who was erwin schrodinger and what did he do?
Australian physicist proposed an equation that incorporated both the wave-like and particle-like behavior of electrons
54
what does the square of wave function do?
gives a probability density map
55
what are orbitals?
wave functions
56
what does n stand for?
principal quantum number
57
what does l stand form?
angular momentum
58
what does ml stand for?
magnetic quantum number
59
what does ms stand for?
spin quantum number
60
what is the principal quantum number
describes the energy level on which the orbital resides
61
what are the values of n?
they are less than 1
62
what is the angular momentum quantum number
defines the shape of the orbital
63
what are the allowed values of l
```
0 to n-1
l = 0
l=1(p)
l=2(d)
l=3(f)
```
64
what is the magnetic quantum number?
describes the 2 d orientation of the orbital
65
what are the allowed values of the magnetic quantum number
-1 to 1 or +- l(everything in between)
66
what are the numbers on the given orbital?
1s, 3p, 5d, 7f
67
what is the value of l for s orbitals
0
68
what is the shape of an s orbital
speherical
69
what happens to the radius when n increases (s orbital)
the radius of the sphere increases because it's more distance away from the nucleus
70
what node does the s orbital possess?
n-1 nodes
71
what is the value of l for the p orbital?
1
72
what is the shape of a p orbital
have two lobes with ai node between them. they look like a dumbell
73
what is the value of l for the d orbital?
2
74
how many lobes does d have
4 lobes
75
what is the shape of the d orbital
the other resembles a p orbital with a doughnut
76
what is the l value for an f orbital?
3
77
what is a spin quantum number?
describes its magnetic field, which affects its energy
78
what is the same thing electrons have regarding spin?
they all have the same spin
79
what was discoverd in the 1920s about spin
two electrons in the same orbital do not have the same energy
80
what orientation can the spin be in?
only in one direction or it's opposite
| spin can be up or down
81
what is the fourth quantum number?
spin quantum or ms
82
what are the two quantum numbers spin has
+1/2 and -1/2
83
who developed the periodic table?
dmitiri mendeleev and lothar meyer came to the conclusion that elements needed to be organized by increasing atomic weight
84
what is periodicity?
repeating chemical and physical properties
85
what was meyers approach to the table?
he believed that the trends were reflective of the internal structure of the elements
86
what was mendeleev's approach to the table
belived in the trend of the table ( perodicity
87
what did mendeleev discover?
germanium, gallium, scandium and he belived that elements were primordial matter
88
what was mendeleev's prediction?
discoveries of gallium and germanium
89
who was henry moseley and what did he do?
developed the concept of atomic numbers
90
how did mosely arrange the elements?
in order of increasing frequencies
91
what are the main group elements
tend to be predictable based on their position in the PT (s and p blocks)
92
are transition element properties more or less predictable
less predictable
93
what is the f block called?
inner transition metals
94
what is the top row of the f block called?
lanthanides
95
what is the bottom of the f block called
actinides
96
why is the f blck similar to the d block
they are both unpredictable
97
what are some characteristics of metals?
shiny luster, solids are malleable and ductile,, good conductors of heat and electricity, most metal oxides are ionic solids that are basic
98
do metals form cations or anions?
cations
99
what is a cation?
ion that will lose an electron (1st group )
100
what is an anion
ion that will gain an electron (7th group)+
101
what are characteristics of nonmetals
do not have shiny luster, , solids are usually brittle, poor conductors of heat, tend to form anios
102
what are metalloids
have characteristics of meals and nonmetals
103
what are some characteristics of metalloids
- semiconductors
| - used in electrical chip
104
what are some metalloids
boron, silicon, germanium, arsenic, antimony, tellurium, astatine
105
what are the components of electron configurations?
number, (n) letter, (l) superscript
106
what is an orbital diagram
another way to represent electron configuration
107
what do the half arrows represent in an orbital diagram
electrons
108
what does the direction of the arrow represent
the relative spin of the electron
109
what does the pauli exclusion principle state?
no two electrons in the same atom have the same energy
- no orbital may have more than 2 electrons and they must have opposite spins
110
what do they say about one electron hydrogen ataom
orbitals on the same principle energy level have the same energy and they degenerate
