Unit 5/Semester Final Flashcards
1
Q
What is the density, mass and volume formula
A
d=m/v
2
Q
Convert 43 miles into feet
A
43(5,280)/1
3
Q
Convert 53 yards per hour into inches per week
A
53(3)(12)(24)(7) / (1)(1)(1)(1)(1)
4
Q
Convert these numbers to scientific notation
450,000 liters
0.000508 kg
A
4.5x10^5
5.08x10^-4
5
Q
Expand these numbers
6.35x10^-5 inches
2.987x10^3 cubits
A
0.0000635
2987
6
Q
Whats the freakin chart?
A
giga 10^9
mega 10^6
kilo 10^3
centi 10^-2
milli 10^-3
micro 10^-6
nano 10^-9
pico 10^-12
7
Q
Convert the following measures into base units expressed in scientific notation
89 megaliters
853,200,000 nanoseconds
A
8.9x10^7
.8532x10^9
8
Q
Whats the rule for sig figs and multiplication and division?
A
the 1st nonzero digit from the left is significant and everything that comes after that is significant
multiply/divide=lowest number of sig figs
add/subtract=lowest number of decimal places
9
Q
perform these operations with correct number of sigfigs
(1.234 kg)(13.1 m/s)
27.34 ft - 5.3241 ft
A
16.2
22.02
10
Q
how many sig figs are in 4.6x10^5
A
6
11
Q
What are the five branches of chemistry
A
Organic
Non-organic
Analytical
Physical
Biochem
12
Q
with carbon
A
organic
13
Q
without carbon
A
non-organic
14
Q
what its made of
A
analytical
15
Q
how it acts
A
physical
16
Q
study of living organisms
A
biochem
17
Q
an educated guess and tries to explain
A
theory
18
Q
just is. and is math
A
law
19
Q
smallest represented particle of an element
A
Atom
20
Q
Whats the law of conservation of mass?
A
in any physical change or chemical reaction, mass is neither created nor destroyed
Lavoisier stated
21
Q
Who came up with the cathode ray tube and what did he discover
A
JJ Thomson
He discovered electrons
22
Q
Who did the gold foil experiment what what did he discover
A
Rutherford
atoms are mostly empty space
23
Q
Draw the gold foil experiment
A
24
Q
Draw the cathode ray tube
A
25
What are the subatomic particles in an atom and their charge?
Proton +
Electron -
Neutron no charge (neutral)
26
Where are the subatomic particles found in an atom
Protons and neutrons in the middle and electrons on the outside
27
Describe how electrons and energy levels are connected
electrons have quantized (set) energy levels that they sit at
28
What did Niels Bohr propose about the atom
it has energy levels
29
valence electrons shown in the group an element is in, largely determine the ______ and _______ properties of an element
chemical and physical
30
The atoms______ ________ determines its placement on the Bohr model
energy level
31
The ________ _________ of an element is the number of protons in the nucleus of an atom. In a neutral atom of an element the number of electrons in the atom________ the number of protons
atomic number
equals
32
The total number of protons and neutrons in an atom is called the _______ ________
mass number
33
What are isotopes
Atoms that have the same number of protons but a different number of neutrons
34
How do you find the atomic mass of an atom
Change % to decimal
multiply by mass (rounded mass number)
add sum together
35
calculate the atomic mass: The isotope with a mass of 10.012 has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%
10.8104973
36
What is the octet rule?
All atoms want 8 valence electrons in order to be stable
37
What are valence electrons
the electrons on the outside or outer shell
38
Identify the groups and periods on a periodic table and what they're significance is
groups tell you the number of valence electrons
periods tell you the number of energy levels
39
Identify the metal, non-metal, liquids, gases, synthetics, alkali, alkali earths, transition metals, halogens, Lanthanides (rare earth), actinides
40
liquids=
gases=
synthetic=
metal=
blue
red
white
black
41
What are the steps to the scientific method
observation/Ask a question
background research
hypothesis
Test experiment
Analyze results/conclusion
Report results
42
What is the Big Bang
The origin of the universe
43
Atomic orbital also known as____is what?
cloud of probability
A three-dimensional region around the nucleus in which an electron can be found
44
What is the quantum mechanical model of an atom?
Limits an electrons energy to certain values and doesn't describe it's path around the nucleus
45
Draw a picture of the quantum mechanical model of an atom
46
What are two shapes in a quantum mechanical model of an atom
s=sphere
p=dumbell
47
Whats the difference between the Bohr and quantum mechanical model of an atom?
Bohr has energy rings and levels whereas the Quantum Mechanical model has clouds of probability
48
Who developed the QM model of the atom
Schrodinger
49
What are the 4 sublevels in the periodic table?
s
p
d
f
50
How many electrons are on the 4th energy level for Tongueston (W)
32 (count everything with a 4 in front until you get to W)
51
Identify the 4 sublevels on the periodic table
52
How many sublevels are in the 3rd energy level
2 (s,p)
53
How many electrons are in an orbital?
2
54
electrons occupy the orbitals of the lowest energy
the aufbau principle
55
an atomic orbital may hold at most 2 electrons to occupy the same orbital, 2 electrons must have opposite spins; that is the electron spins must be paired
pauli exclusion principle
56
when electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain 1 electron with parallel spin
Hund's rule
57
Write long hand electron configuration for these
hydrogen
bromine
arsenic
1s^1
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^3
58
Identify the element that corresponds to each of the following
1s^2 2s^2 2p^3
1s^2 2s^2 2p^4
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2
N
O
Ti
59
Write the following in shorthand
carbon
potassium
iodine
[He] 2s^2 2p^2
[Ar] 4s^1
[Kr] 5s^2 4d^10 5p^5
60
Determine the number of unpaired electron
Lithium
nickel
manganese
1
2
5
61
Atomic size generally______as you go down a group and generally______as you move from left to right along a period on the periodic table
increases
decreases
62
The shielding effect generally______as you go down a group and generally______as you move from left to right along a period on the periodic table
increases
little to no effect
63
electronegativity generally______as you go down a group and generally______as you move from left to right along a period on the periodic table
decreases
increases
64
Whats an ion and how do you know if its a cation or anion
a charged particle
Cations are metals, positive and smaller
Anions are non-metals, negative and are bigger
65
distance between the crests
wavelength (y)
66
waves height from origin to the crests
amplitude
67
What's the equation for frequency and wavelength
c=yv
68
Whats the relationship between energy, frequency and wavelength
e=hv
shorter wavelength+high frequency=greater energy
long wavelength+low frequency=lower energy
69
E=
h x v
70
how is light emitted from atoms
photons
71
what is a quanta of light and another name for it
a pocket of light, photon
72
a packet of energy released when an electron falls back down from excited state to ground state
photon
73
Draw the electromagnetic spectrum
74
draw the visible light spectrum
75
how is the speed of light affected by energy and wavelength
it doesn't change/stays the exact same speed no matter what
76
An inexpensive laser that is available to public emits light that has a wavelength of 670 nm
1. Whats the frequency
2. whats the energy
1. 4.478^14
2.9671228^-18
77
-an atom with an electron in the ground state and when the electron gets excited it changes to an excited state and it falls back down to the ground state and emits a photon that produces the lights we see in the AES
-When light emitted from the atom is passed through a prism it produces discrete lines corresponding to the frequencies of light that was emitted from that atom
Atomic Emission spectrum
78
What do the different colors tell us about what is happening with the electrons in the Atomic emission spectrum
Shorter wavelength=more energy
longer wavelength=less energy
The amount of energy released from where the atom fell from excited to ground state
79
the process by which unstable atomic nuclei achieve stability
radioactivity
80
the penetrating rays and particles emitted by a radioactive source
radiation
81
an isotope that has an unstable atomic nucleus that undergoes radioactive decay
radioisotope
82
the spontaneous emission of radiation by an unstable nucleus, the rate of decay is unaffected by temperature, pressure,or catalyst
radioactive decay
83
what is the purpose if radioactive decay and what will it result in
to reach a more stable state
a stable isotope
84
Nuclear Chemistry
Chemistry that takes place in the nucleus
85
What particles are involved in a fission reaction and what particles are produced
its hit with neutrons
it produces two nuclei and more neutrons
86
what particles are involved in a fusion reaction and what particles are produced
in solar fusion hydrogen nuclei (protons) fuse to produce helium nuclei and two positron this results in LOTS of energy and more then fission
87
Whats the force that holds the nucleus together and is the strongest force in the universe?
strong nuclear force
88
write the symbol and charge of the three types of decay
Alpha 4/2He a(fish)
Beta 0/-1e B
Gamma 0 y
89
The time required for one half of the atoms of a radioisotope to emit radiation and decay to products
half-life
90
How do u find the product of electron capture
PUT ON THE LEFT!!
0/-1e
91
How is a positron similar/different from an electron
It has the same mass but a positive charge
92
How do u find the product of positron emission
0/+1e
93
What are the patterns for alpha, beta and gamma radiation
alpha= decrease by 2
beta= increases by 1
gamma= stays same
94
How do you add to a radioisotope for beta radiation
0/-1e
95
What are the penetrating powers of alpha beta and gamma radiation
smallest------------------------------------------>largest
alpha beta gamma
96
What do you add to a radioisotope for alpha radiation
4/2 He
97
Write a nuclear equation to represent Alpha decay
238
Pu
94
234 4
U He
92 2
98
Write the equation for beta decay
Carbon-14
14/7N + 0/-1e
99
Write the equation for electron capture
16/8O
0/-1e-----------------------> 16/7N
100
Write the equation for positron emission
80/35Br
0/+1e + 80/34Se
101
The Half-life of tritium is 12.3 year. If 48.o mg of tritium is released from a nuclear power plant during the course of a mishap, what mass of tritium will remain after 49.2 yr?
3
102
Practice a naming sheet
103
Draw the electron dot structure of the following molecules
02
N2
104
Nonpolar covalent bond
atoms pull equally as occurs when identical atoms are bonded
105
polar covalent bond
atoms are unequally shared
106
The bigger side of a polar bond is ______ and the smaller side is ______
-
+
107
dipole
molecule has two pulls (+ , -)
108
Ionic compounds are______ and covalent are_______
metals
non-metals
109
good conductors of heat and electricity, ductile, malleable
properties of metal
110
most are gases, not good conductors of heat and electricity
properties of nonmetal
111
Write the lewis dot structure for H3O^+
112
Write the lewis dot structure for SO3^2-
113
Write electron dot diagram for 02 and N2
114
What are the measurements for Volume, Mass, and Density
liters, grams, grams per liters
115
electrons are in ____ of________
clouds of probability
116
When an electron falls down from its excited state to ground state it __________energy
loses
117
The atomic number only tells you the number of ____
protons
118
How many orbitals does the s sublevel have
1
119
How many orbitals does the p sublevel have
3
120
how many orbitals does the d sublevel have
5
121
How many orbitals does the f sublevel have
7
122
Electronegativity increases as you get closer to _______
Fluorine
123
Which one is an anion and cation
Cl-
Sr+2
anion
cation
124
Draw the parts of a wave
draw trough, crest, and wavelength
125
What is CH4
methane
126
What is NH3
Ammonia
127
What is H2O
water
128
When its a non-metal paired with another non-metal then ______ ________ whereas when its a metal paired with a non-metal then _____
don't simplify
simplify
129
Write the charge and criss cross_________.
always
130
How many valence electrons does Hydrogen want to have?
2
131
define ionic, molecular, and acid
metal, non-metal, H or acid
132
methane
CH4
133
ammonia
NH3
