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Chemistry > Unit 5/Semester Final > Flashcards

Unit 5/Semester Final Flashcards

1
Q

What is the density, mass and volume formula

A

d=m/v

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2
Q

Convert 43 miles into feet

A

43(5,280)/1

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3
Q

Convert 53 yards per hour into inches per week

A

53(3)(12)(24)(7) / (1)(1)(1)(1)(1)

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4
Q

Convert these numbers to scientific notation
450,000 liters
0.000508 kg

A

4.5x10^5
5.08x10^-4

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5
Q

Expand these numbers
6.35x10^-5 inches
2.987x10^3 cubits

A

0.0000635
2987

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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

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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

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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

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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

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10
Q

how many sig figs are in 4.6x10^5

A

6

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11
Q

What are the five branches of chemistry

A

Organic
Non-organic
Analytical
Physical
Biochem

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12
Q

with carbon

A

organic

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13
Q

without carbon

A

non-organic

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14
Q

what its made of

A

analytical

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15
Q

how it acts

A

physical

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16
Q

study of living organisms

A

biochem

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17
Q

an educated guess and tries to explain

A

theory

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18
Q

just is. and is math

A

law

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19
Q

smallest represented particle of an element

A

Atom

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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

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21
Q

Who came up with the cathode ray tube and what did he discover

A

JJ Thomson
He discovered electrons

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22
Q

Who did the gold foil experiment what what did he discover

A

Rutherford
atoms are mostly empty space

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23
Q

Draw the gold foil experiment

A
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24
Q

Draw the cathode ray tube

A
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25
Q

What are the subatomic particles in an atom and their charge?

A

Proton +
Electron -
Neutron no charge (neutral)

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26
Q

Where are the subatomic particles found in an atom

A

Protons and neutrons in the middle and electrons on the outside

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27
Q

Describe how electrons and energy levels are connected

A

electrons have quantized (set) energy levels that they sit at

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28
Q

What did Niels Bohr propose about the atom

A

it has energy levels

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29
Q

valence electrons shown in the group an element is in, largely determine the ______ and _______ properties of an element

A

chemical and physical

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30
Q

The atoms______ ________ determines its placement on the Bohr model

A

energy level

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31
Q

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

A

atomic number
equals

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32
Q

The total number of protons and neutrons in an atom is called the _______ ________

A

mass number

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33
Q

What are isotopes

A

Atoms that have the same number of protons but a different number of neutrons

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34
Q

How do you find the atomic mass of an atom

A

Change % to decimal
multiply by mass (rounded mass number)
add sum together

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35
Q

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%

A

10.8104973

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36
Q

What is the octet rule?

A

All atoms want 8 valence electrons in order to be stable

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37
Q

What are valence electrons

A

the electrons on the outside or outer shell

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38
Q

Identify the groups and periods on a periodic table and what they’re significance is

A

groups tell you the number of valence electrons
periods tell you the number of energy levels

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39
Q

Identify the metal, non-metal, liquids, gases, synthetics, alkali, alkali earths, transition metals, halogens, Lanthanides (rare earth), actinides

A
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40
Q

liquids=
gases=
synthetic=
metal=

A

blue
red
white
black

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41
Q

What are the steps to the scientific method

A

observation/Ask a question
background research
hypothesis
Test experiment
Analyze results/conclusion
Report results

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42
Q

What is the Big Bang

A

The origin of the universe

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43
Q

Atomic orbital also known as____is what?

A

cloud of probability
A three-dimensional region around the nucleus in which an electron can be found

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44
Q

What is the quantum mechanical model of an atom?

A

Limits an electrons energy to certain values and doesn’t describe it’s path around the nucleus

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45
Q

Draw a picture of the quantum mechanical model of an atom

A
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46
Q

What are two shapes in a quantum mechanical model of an atom

A

s=sphere
p=dumbell

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47
Q

Whats the difference between the Bohr and quantum mechanical model of an atom?

A

Bohr has energy rings and levels whereas the Quantum Mechanical model has clouds of probability

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48
Q

Who developed the QM model of the atom

A

Schrodinger

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49
Q

What are the 4 sublevels in the periodic table?

A

s
p
d
f

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50
Q

How many electrons are on the 4th energy level for Tongueston (W)

A

32 (count everything with a 4 in front until you get to W)

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51
Q

Identify the 4 sublevels on the periodic table

A
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52
Q

How many sublevels are in the 3rd energy level

A

2 (s,p)

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53
Q

How many electrons are in an orbital?

A

2

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54
Q

electrons occupy the orbitals of the lowest energy

A

the aufbau principle

55
Q

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

A

pauli exclusion principle

56
Q

when electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain 1 electron with parallel spin

A

Hund’s rule

57
Q

Write long hand electron configuration for these
hydrogen
bromine
arsenic

A

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
Q

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

A

N
O
Ti

59
Q

Write the following in shorthand
carbon
potassium
iodine

A

[He] 2s^2 2p^2
[Ar] 4s^1
[Kr] 5s^2 4d^10 5p^5

60
Q

Determine the number of unpaired electron
Lithium
nickel
manganese

A

1
2
5

61
Q

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

A

increases
decreases

62
Q

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

A

increases
little to no effect

63
Q

electronegativity generally______as you go down a group and generally______as you move from left to right along a period on the periodic table

A

decreases
increases

64
Q

Whats an ion and how do you know if its a cation or anion

A

a charged particle
Cations are metals, positive and smaller
Anions are non-metals, negative and are bigger

65
Q

distance between the crests

A

wavelength (y)

66
Q

waves height from origin to the crests

A

amplitude

67
Q

What’s the equation for frequency and wavelength

A

c=yv

68
Q

Whats the relationship between energy, frequency and wavelength

A

e=hv
shorter wavelength+high frequency=greater energy
long wavelength+low frequency=lower energy

69
Q

E=

A

h x v

70
Q

how is light emitted from atoms

A

photons

71
Q

what is a quanta of light and another name for it

A

a pocket of light, photon

72
Q

a packet of energy released when an electron falls back down from excited state to ground state

A

photon

73
Q

Draw the electromagnetic spectrum

A
74
Q

draw the visible light spectrum

A
75
Q

how is the speed of light affected by energy and wavelength

A

it doesn’t change/stays the exact same speed no matter what

76
Q

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

A
  1. 4.478^14
    2.9671228^-18
77
Q

-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

A

Atomic Emission spectrum

78
Q

What do the different colors tell us about what is happening with the electrons in the Atomic emission spectrum

A

Shorter wavelength=more energy
longer wavelength=less energy
The amount of energy released from where the atom fell from excited to ground state

79
Q

the process by which unstable atomic nuclei achieve stability

A

radioactivity

80
Q

the penetrating rays and particles emitted by a radioactive source

A

radiation

81
Q

an isotope that has an unstable atomic nucleus that undergoes radioactive decay

A

radioisotope

82
Q

the spontaneous emission of radiation by an unstable nucleus, the rate of decay is unaffected by temperature, pressure,or catalyst

A

radioactive decay

83
Q

what is the purpose if radioactive decay and what will it result in

A

to reach a more stable state
a stable isotope

84
Q

Nuclear Chemistry

A

Chemistry that takes place in the nucleus

85
Q

What particles are involved in a fission reaction and what particles are produced

A

its hit with neutrons
it produces two nuclei and more neutrons

86
Q

what particles are involved in a fusion reaction and what particles are produced

A

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
Q

Whats the force that holds the nucleus together and is the strongest force in the universe?

A

strong nuclear force

88
Q

write the symbol and charge of the three types of decay

A

Alpha 4/2He a(fish)
Beta 0/-1e B
Gamma 0 y

89
Q

The time required for one half of the atoms of a radioisotope to emit radiation and decay to products

A

half-life

90
Q

How do u find the product of electron capture

A

PUT ON THE LEFT!!
0/-1e

91
Q

How is a positron similar/different from an electron

A

It has the same mass but a positive charge

92
Q

How do u find the product of positron emission

A

0/+1e

93
Q

What are the patterns for alpha, beta and gamma radiation

A

alpha= decrease by 2
beta= increases by 1
gamma= stays same

94
Q

How do you add to a radioisotope for beta radiation

A

0/-1e

95
Q

What are the penetrating powers of alpha beta and gamma radiation

A

smallest——————————————>largest
alpha beta gamma

96
Q

What do you add to a radioisotope for alpha radiation

A

4/2 He

97
Q

Write a nuclear equation to represent Alpha decay
238
Pu
94

A

234 4
U He
92 2

98
Q

Write the equation for beta decay
Carbon-14

A

14/7N + 0/-1e

99
Q

Write the equation for electron capture
16/8O

A

0/-1e———————–> 16/7N

100
Q

Write the equation for positron emission
80/35Br

A

0/+1e + 80/34Se

101
Q

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?

A

3

102
Q

Practice a naming sheet

A
103
Q

Draw the electron dot structure of the following molecules
02
N2

A
104
Q

Nonpolar covalent bond

A

atoms pull equally as occurs when identical atoms are bonded

105
Q

polar covalent bond

A

atoms are unequally shared

106
Q

The bigger side of a polar bond is ______ and the smaller side is ______

A

-
+

107
Q

dipole

A

molecule has two pulls (+ , -)

108
Q

Ionic compounds are______ and covalent are_______

A

metals
non-metals

109
Q

good conductors of heat and electricity, ductile, malleable

A

properties of metal

110
Q

most are gases, not good conductors of heat and electricity

A

properties of nonmetal

111
Q

Write the lewis dot structure for H3O^+

A
112
Q

Write the lewis dot structure for SO3^2-

A
113
Q

Write electron dot diagram for 02 and N2

A
114
Q

What are the measurements for Volume, Mass, and Density

A

liters, grams, grams per liters

115
Q

electrons are in ____ of________

A

clouds of probability

116
Q

When an electron falls down from its excited state to ground state it __________energy

A

loses

117
Q

The atomic number only tells you the number of ____

A

protons

118
Q

How many orbitals does the s sublevel have

A

1

119
Q

How many orbitals does the p sublevel have

A

3

120
Q

how many orbitals does the d sublevel have

A

5

121
Q

How many orbitals does the f sublevel have

A

7

122
Q

Electronegativity increases as you get closer to _______

A

Fluorine

123
Q

Which one is an anion and cation
Cl-
Sr+2

A

anion
cation

124
Q

Draw the parts of a wave

A

draw trough, crest, and wavelength

125
Q

What is CH4

A

methane

126
Q

What is NH3

A

Ammonia

127
Q

What is H2O

A

water

128
Q

When its a non-metal paired with another non-metal then ______ ________ whereas when its a metal paired with a non-metal then _____

A

don’t simplify
simplify

129
Q

Write the charge and criss cross_________.

A

always

130
Q

How many valence electrons does Hydrogen want to have?

A

2

131
Q

define ionic, molecular, and acid

A

metal, non-metal, H or acid

132
Q

methane

A

CH4

133
Q

ammonia

A

NH3

Chemistry (17 decks)

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