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Chemistry 100 SDSU > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

Are pure substances visible to our naked eye?

A

No, we talk about it at the submicroscopic level

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2
Q

Are Mixtures visible to our naked eye?

A

Yes, we talk about it at the microscopic level

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3
Q

What are the two types of pure substances?

A

Elements and Compounds

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4
Q

What are the two types of mixtures?

A

Heterogeneous or Homogeneous

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5
Q

What is the difference between an elements and a compound?

A

An Element is a singular composition of matter (elements form the periodic table)
A compound is made up of these elements

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6
Q

What is the difference between a homogeneous and heterogeneous mixture?

A

Homogeneous is a mixture that has a uniform appearance.
EX: salt and sugar
Heterogeneous is a mixture that has a visible variety of substances
EX: salt and pepper

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7
Q

What are the types of properties?

A

Physical and chemical

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8
Q

What is part of a physical property?

A

it can include appearance, density, solubility, freezing point, boiling point

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9
Q

How do we know a property is physical?

A

Physical properties do NOT change the identity of the substance

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10
Q

What is part of a chemical property?

A

Flammability and Reactivity

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11
Q

What determines a property as a chemical one?

A

Chemical changes convert one substance into another

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12
Q

What type of measurement system do we use in science?

A

The Metric System

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13
Q

In sig figs ________ always count

A

Integers

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14
Q

Do zeros in between 2 integers count? Provide an example

A

Yes, zeros in between two integers ALWAYS count

ex: 12,004

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15
Q

Do zeros in the beginning of a number count? Provide an example..

A

No, zeros in the beginning of a number NEVER count

ex: 0.000015

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16
Q

Zeros at the end only count if and only if…

A

there is a decimal

ex: 1,200.56

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17
Q

What do we know about zeros that are at the end but before a decimal?

A

We are unsure of whether or not they count

ex: 100

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18
Q

When calculating sig. figs, (addition and subtraction), what are the rules?

A

Your final answer can only have as many decimal places as the least exact measurement.
ex: 3.18 + 0.01315 means your answer can only have 6 decimal places since 0.01315 is the LEAST exact measurement

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19
Q

When calculating sig. figs, (multiplication and division), what are the rules?

A

Your final answer can only have as many SIG FIGS as the least exact measurement.
ex: 203 * 0.0048 means your answer can only have 2 sig figs since 0.0048 has the LEAST exact measurement.

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20
Q

What contents are in scientific notation?

A

It contains a coefficient and an exponential notation (*10 ^ x)

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21
Q

If the exponent in the notation is positive, where do we move the decimal?

A

to the right

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22
Q

If the exponent in the notation is negative, where do we move the decimal?

A

To the left

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23
Q

What are the 3 conversion factors for grams?

A

1 kg = 1000 g
1mg = 0.001 g
1000 mg = 1 g

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24
Q

How do you convert from Celsius to Kelvin?

A

K= Celsius + 273

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25
Q

How do you convert Kelvin to Celsius

A

Celsius= K - 273

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26
Q

How do you convert Farenheit to Kelvin?

A
  1. Convert Farenheit to Celsius
    Celsius = (F - 32) * (5/9)
  2. Use the celsius to convert to Kelvin
    Celsius +273
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27
Q

How do you convert Kelvin to Farenheit?

A
  1. Convert Kelvin to Celsius by subtracting 273
  2. Use that value to find farenheit
    Celsius * (9/5) + 32
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28
Q

What is the formula for specific heat?

A

heat / (mass) ( change in temp)
OR
(J)/ (g * Change in Celsius)

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29
Q

What is the notation (from class) to write an atom

includes mass # and atomic #

A

[ mass #]

[ Atomic # } X

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30
Q

What is an isotope?

A

These occur when atoms of the same element contain different numbers of neutrons

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31
Q

What is an ion?

A

An ion is formed when an atom (or groups of atoms) has either a +/- charge due to their number of electrons

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32
Q

If we have too many electrons we have a/an _______. It has a __________ charge

A

Anion/ negative

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33
Q

If we have too few electrons, we have a/an _________. It has a ___________ charge

A

Cation/ positive

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34
Q

Which periodic group is more likely to lose electrons?

Metals/non metals/ halogens/ noble gases

A

metals

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35
Q

Which periodic groups is more likely to gain electrons?

A

Non metals

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36
Q

How do you solve for atomic mass?

A

First separate the isotopes with their corresponding percentage. Then multiply their individual mass with their percent. Lastly, add the two values in order to get your average atomic mass.

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37
Q

How do you solve for mass percent?

A

You simply divide the mass of the element by the total mass and then multiply by 100

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38
Q

What is Daltons Atomic Theory

A
  1. All matter is made from indivisible particles called atoms
  2. Atoms of the same element are chemically identical
  3. Elements are characterized by the mass of their atoms
  4. Atoms join in small whole number ratios to form compounds
  5. Reactions change the combination of atoms not the atoms themselves
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39
Q

How is Dalton’s Atomic Theory a bit outdated?

A

Although atoms are indivisible particles, we know that something makes up those atoms (protons, neutrons and electrons)
We also know that atoms of the same element can have different masses due to their number of neutrons

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40
Q

All types of light and radiations fall along the ___________ spectrum

A

electromagnetic

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41
Q

What is the order of lowest energy to highest?

A

Radio waves, microwaves, Infarred, Ultraviolet, X Rays and Gamma Rays

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42
Q

Particles of light are called

A

Photons

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43
Q

How dies Atomic Spectra help our understanding of electron energy.

A

This helps us understand that electron energy is quantized. The specific colors associated with atoms is due to the amount of energy level.

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44
Q

What do we mean by quantized?

A

This means there is only a specific amount of energy allowed for every electron

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45
Q

t/f Electrons follow definite circular paths

A

false, they are mainly in a diffused cloud of negative charge around the nucleus

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46
Q

t/f atomic orbitals are NOT solids

A

true, orbitals are simply areas in which an electron will most likely be located

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47
Q

How are orbitals described?

A

Based on their energy level

48
Q

What are the 3 types of subshells

A

s,p,d

49
Q

A subshell has a specific amount of _______ while each of those has exactly ____ electrons.

A

Orbital, 2

50
Q

How many orbitals does the S subshell have

A

one orbital (it goes by one) (2 electrons)

51
Q

How many orbitals does the P subshell have? How many electrons total?

A

3 orbitals (6 electrons)

52
Q

How many orbitals does the D subshell have?

A

5 orbitals (10 electrons)

53
Q

The P subshell only shows up after energy level ___. The D subshell only shows up after energy level ____.

A

2,3

54
Q

What is the ground state electron configuration?

A

1s,2s,2p,3s,3p,4s, 3d, 4p

55
Q

What is the condensed electron configuration?

A

It is when we use the nearest noble gas to the element were dealign with (without surpassing it) and writing the rest of the electron configuration after that.

56
Q

Group 1 (Column) is what type of elements?

A

Alkali metal

57
Q

Group 2 of the PT has what type of elements?

A

Alkaline Earth Metals

58
Q

Group 7 of the PT has what type of elements?

A

Halogens

59
Q

Group 8 of the PT has what type of elements?

A

Noble Gases

60
Q

Overall, where are the metals located at (in the PT)?

A

The left hand side/middle

61
Q

Overall, where are the non-metals located at in the PT

A

The right hand side

62
Q

What is electronegativity?

A

It is basically a description of how much strength an atom has to pull electrons towards themselves.

63
Q

Which element has the highest electronegativity value?

A

Fluorine

64
Q

When we have 2 atoms with similar electronegativity value, what happens to the electrons/

A

They are shared equally (non-polar covalent bond)

65
Q

When we have 2 atoms with different electronegativity values, what happens to electrons

A

They are shared unequally and we have a polar covalent bond

66
Q

As long as electrons are shared, the bond is _______-

A

Covalent

67
Q

What is an ionic bond?

A

A complete transfer of electrons due to the differences in electronegativity values

68
Q

Covalent/ Ionic will always have discrete units, will only ever have the amount it specifies

A

Covalent

69
Q

An ionic bond usually contains which 2 periodic table groups?

A

Metals and Non-metals

70
Q

What are the rules for naming REGULAR ionic bonds?

A

The cation (metal) keeps its name but the non-metal’s ending changes to ide

71
Q

What are the rules for naming POLYATOMIC ions?

A

They will always keep their name

72
Q

A covalent bond ONLY contains which periodic table group?

A

Non metals

73
Q

What are the rules for naming covalent bonds?

A

The ending of the 2nd element changed to ide and both elements use prefixes (except for mono on the first element)

74
Q

What are the 7 diatomic molecules?

A

Nitrogen, Oxygen, Chlorine, Bromine, Fluoride, Iodine and Hydrogen

75
Q

Why should we watch out for diatomic molecules in covalent bonds?

A

Because these element always come in pairs and they retain their name

76
Q

What is a Binary Ionic Compound

A

It is a compound that only contains 2 elements (cation and anion)

77
Q

What should be the charge of a Binary Ionic Compound?

A

0, it must always be balanced and canceled out

78
Q

Why are the naming rules different for Ionic Transition metals?

A

Because some of the transition metals can have multiple charges

79
Q

What are the 2 charges of Chromium?

A

Cr2+ and Cr3+

80
Q

What are the 2 charges of Iron?

A

Fe2+ and Fe3+

81
Q

What are the charges of Copper?

A

Cu+ and Cu 2+

82
Q

What are the 2 charges of Tin?

A

Sn2+ and Sn4+

83
Q

What are the 2 charges of Mercury?

A

Hg2^2 (diatomic) + and Hg2+

84
Q

What are the 2 charges of Thallium?

A

Tl+ and Tl3+

85
Q

What are the 2 charges of Lead?

A

Pb2+ and Pb4+

86
Q

What are the rules for ionic polyatomic ions?

A

Metals keep their name but we add roman numerals to desceribe the charge.

87
Q

What should we make sure of when naming bonds?

A

make sure they are balanced out

88
Q

________ substances are NON ELECTROLYTES

A

Covalent

89
Q

What is the prefix for one?

A

Mono

90
Q

What is the prefix for 2?

A

Di

91
Q

What is the prefix for 3?

A

Tri

92
Q

What is the prefix for 4?

A

Tetra

93
Q

What is the prefix for 5?

A

Penta

94
Q

What is the prefix for 6?

A

Hexa

95
Q

What is the prefix for 7?

A

Hepta

96
Q

What is the prefix for 8?

A

Octa

97
Q

What is the prefix for 9?

A

Nona

98
Q

What is the prefix for 10?

A

Deca

99
Q

ALL acids contain which cation?

A

H+

100
Q

How do we distinguish acids from other substances?

A

Hydrogen will be written first

101
Q

If we have binary acids, what are the rules?

A

Hydro will be the prefix and we will add -ic and acid to the ending

102
Q

If we have polyatomic acids, what are the rules?

A

No hydro prefix
ate ending becomes ic
ite ending becomes ous
add acid at the end

103
Q

For electron geo., if there are 2 things around the central atom and 2 bonds, what are the 2 forms of geometry and angle

A

linear, linear, 180

104
Q

For electron geo., if there are 3 things around the central atom and 3 bonds, what are the 2 forms of geometry and angle

A

Trigonal planar, trigonal planar, 120

105
Q

For electron geo., if there are 3 things around the central atom and 2 bonds, what are the 2 forms of geometry and angle

A

Trigonal planar, bent, <120

106
Q

For electron geo., if there are 4 things around the central atom and 4 bonds, what are the 2 forms of geometry and angle?

A

tetrahedral, tetrahedral 109.5

107
Q

For electron geo., if there are 4 things around the central atom and 3 bonds, what are the 2 forms of geometry and angle

A

Tetrahedral, trigonal pyramid <109.5

108
Q

For electron geo., if there are 4 things around the central atom and 2 bonds, what are the 2 forms of geometry and angle?

A

Tetrahedral, bent, <109.5

109
Q

For electron geometry, what is considered a “thing” around the central atom?

A

A single bond
A double bond
A triple Bond
A lone pair

110
Q

Why do we have different molecular geometries?

A

When we have lone pairs instead of bonds, the molecular geometry will be different than electron geometry because lone pairs are simply taking up space. They are not connected to atoms

111
Q

atoms closer to ______ have higher electronegativity values

A

Fluorine

112
Q

In order to be a polar molecule, what has to happen?

A

We have to have polar bonds (unequal sharing of electrons) that are not symmetrical

113
Q

When solving for unit conversions, the units to the right of the base are (-) or +

A

Negative
K H D B D C M

B= base and everything to the right of it is negative

114
Q

What are the 2 forms of acids?

A

One with oxygen and one without

115
Q

When you have an acid with oxygen, does it have a prefix?

A

No

116
Q

When you have an acid without oxygen, do you have a prefix?

A

yes you add hydro to the front

Chemistry 100 SDSU (5 decks)

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