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Chemistry 100 SDSU > Final Exam > Flashcards

Final Exam Flashcards

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1
Q

How do we determine if substance is a pure substance?

A

When we talk about a pure substances we refer to the submicroscopic level

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2
Q

How do we determine if a substance is a mixture?

A

Mixtures are visible to us (macroscopic level)

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3
Q

Within pure substances we have…

A

elements and compounds

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4
Q

Withing mixtures, we have…

A

homogenous mixtures and heterogeneous mixtures

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5
Q

What are the 2 types of properties?

A

Physical and chemical

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6
Q

What is the difference between physical and chemical?

A

physical properties include: density,mass appearance, color, freezing/boiling point.
Chemical properties include: flammability, reactivity (chemical changes convert one substance into another, physical does not)

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7
Q

What are the rules for sig figs in addition and subtraction?

A

Our answer has as many decimal places as the least exact measurement

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8
Q

What are the rules for sig figs in multiplication and division?

A

Your answer has as many sig figs as the least exact measurement

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9
Q

What are the rules for sig figs in logs?

A

The number of sig figs in the parenthesis (starting value) equals the number of decimal places
ex: log(4.1 * 10^-3) = 2.39

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10
Q

What are the rules for sig figs in antilogs?

A

The number of decimal places in the antilog equals the number of sig figs in the result
ex: antilog (1.325)= 10^1.325= 21.1

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11
Q

How do we find celsius given Fahrenheit

A

C = (F-32) * 5/9

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12
Q

How do we find Fahrenheit given celsius?

A

F = C * 9/5 + 32

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13
Q

How do we find Kelvin?

A

If we are given Celsius just add 273. If we are given Fahrenheit simply convert to celsius first and then add 273

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14
Q

What is specific heat?

A

It measures the ability of a substance to absorb heat

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15
Q

What is the formula of specific heat?

A

(Heat) / mass * change in temp.

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16
Q

What happens if we change the number of protons?

A

We change the element

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17
Q

What happens if we change the number of neutrons? What does it form?

A

We change the mass forming an isotope

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18
Q

What happens if we change the number of electrons? What does it form?

A

We change the charge of an element forming an ion

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19
Q

Elements are identified by their _____ which is equal to the number of protons

A

Atomic number

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20
Q

How do we write the notation for an element?

A

(Mass on top) (atomic number on bottom) and element symbol on the right

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21
Q

What are the two types of ions?

A

Cations and Anions

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22
Q

What is a cation?

A

It has a positive charge and it is formed by losing electrons

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23
Q

Which group of elements are most likely to be cations?

A

metals

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24
Q

What is an anion?

A

A negatively charge element formed by gaining electrons.

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25
Q

Which group of elements are most likely to be anions?

A

non-metals

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26
Q

How do we calculate average atomic mass?

A

Since we are given two isotopes and their percent of abundance, take the corresponding percentage of their atomic mass and add.

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27
Q

What is the law of constant composition?

A

Elements always combine in the same proportion and formula.

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28
Q

How do we find mass percent?

A

(part/whole) * 100

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29
Q

How is Daltons Atomic Theory outdated?

A

It stated that atoms of the same element were the same mass and atoms of different elements had different mass.

All matter is made of indivisible particles called atoms

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30
Q

Atomic Spectra helps us understand that electron energy is…

A

quantizied

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31
Q

The areas where an electron will most likely be is called a

A

orbital

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32
Q

Orbitals have a __ % probability

A

90%

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33
Q

What are the 3 types of subshells and how many orbitals do each have?

A

S subshells have 1 orbital
p subshells have 3 orbitals
d subshells have 5 orbitals

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34
Q

Each orbital can hold how many electrons?

A

2

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35
Q

What is the ground state electron configuration?

A

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

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36
Q

Alkali metals are in group _
Alkaline metals are in group _
Halogens are in group _
Noble gases are in group _

A

Alkali metals are in group 1
Alkaline metals are in group 2
Halogens are in group 7
Noble gases are in group 8

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37
Q

What is electronegativity?

A

It is a value that describes the extent to which atoms pull electrons.

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38
Q

Which element has the highest electronegativity value?

A

Fluorine

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39
Q

Which group has overall higher electronegativity values?

A

Nonmetals, they are more likely to pull electrons toward themselves

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40
Q

What is a non-polar covalent bond?

A

When we have 2 atoms that have a similar or identical electronegativity value, electrons are shared equally

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41
Q

What is a polar covalent bond?

A

When we have 2 different electronegativity values between atoms, sharing is unequal

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42
Q

The sharing of electrons is what type of bond?

A

Covalent

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43
Q

What is an ionic bond?

A

When electrons are completely transferred due to the difference in electronegativity values

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44
Q

What are the rules for naming ionic bonds?

A 
The cation (metal) retains its name and the nonmetal's ending changes to -ide
The only exception is polyatomic ions (retain their name)
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45
Q

What are the rules for naming covalent bonds?

A

The ending of the second element will change to-ide.
Covalent compounds always use prefixes (except for mono on first)
The only exception to this is diatomic molecules (they retain their name)

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46
Q

What are the 7 diatomic elements?

A

Hydrogen, Oxygen, Fluorine, Chlorine, Nitrogen, Iodine, Bromine

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47
Q

Why do we have to memorize transition metal charges?

A

Because they arent predictable

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48
Q

What are the charges for Chromium? (Cr)

A

2+ and 3+

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49
Q

What are the charges for Iron? (Fe)

A

2+ and 3+

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50
Q

What are the charges for copper? (Cu)

A

1+ and 2+

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51
Q

What are the charges for mercury? (Hg)

A

Hg(2) 2+ and 2+

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52
Q

What are the charges for tin? (Sn)

A

2+ and 4+

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53
Q

What are the charges for lead? (Pb)

A

2+ and 4+

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54
Q

How do we name binary compounds with transition metals?

A

No prefixes
Metals retain name, nonmetal changes to ide
Roman numerals are needed for the charge

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55
Q

How do we name covalent molecules?

A 
Add prefixes (except for mono on first element) 
2nd element ending changes to ide 
Diatomic molecules retain their name
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56
Q

What are the first 10 prefixes?

A

1: mono
2: di
3: tri
4: tetra
5: penta
6: hexa
7: hepta
8: octa
9: nona
10: deca

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57
Q

How do we know if a substance is an acid?

A

It will have an H in the beginning of the formula

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58
Q

What are the rules for binary acids?

A

Prefix will be hydro
Second element becomes ic
Add acid at end
EX: hydrochloric acid = HCl

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59
Q

What are the rules for polyatomic acids?

A 
No Hydro prefix
If ending was ate it turns to ic 
If ending was ite it turns to ous
Add acid 
EX: H2SO4= sulfuric acid
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60
Q

If there are 2 bonds around the central atom the electron geometry is _______, the molecular geometry is _______. The bond angle is _______

A

Linear, Linear, 180

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61
Q

If there are 3 things around the central atom but only 2 bonds, the electron geometry is ______, the molecular geometry is _______. The bond angle is ______

A

trigonal planar, bent, <120

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62
Q

If there are 3 things around the central atom and 3 bonds, the electron geometry is ______, the molecular geometry is _______. The bond angle is _______

A

trigonal planar, trigonal planar, 120

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63
Q

If there are 4 things around the central atom but only 3 bonds, the electron geometry is ______, the molecular geometry is _______. The bond angle is _____

A

tetrahedral, trigonal pyramidal, <109.5

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64
Q

If there are 4 things around the central atom but only 2 bonds, the electron geometry is ______, the molecular geometry is _______. The bond angle is _______

A

tetrahedral, bent, <109.5

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65
Q

If there are 4 things around the central atom and 4bonds, the electron geometry is ______, the molecular geometry is _______. The bond angle is _______

A

tetrahedral, tetrahedral, 109.5

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66
Q

How do we know if a compound is polar?

A

We compare their electronegativity values, draw a lewis structure and make sure the molecule’s polarity isn’t canceled by symmetry.

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67
Q

How is symmetry unbalanced in a bond?

A

When we have lone pairs around central atom or when there are no identical groups around it.

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68
Q

What is the law of conservation of mass?

A

Even though reactions convert reactants to products, there still is the same number and type of product

69
Q

One mole = ?

A

6.022 *10 ^-23 atoms/particles

70
Q

What is molar mass?

A

The sum of all elements in a compound

71
Q

We go from moles to atoms using

A

Avogadros Number

72
Q

We go from moles to grams by

A

using molar mass

73
Q

We go from moles to moles by

A

using coefficients from balanced equation

74
Q

What is the difference of empirical formula and molecular formula?

A

An empirical formula represents the formula of a compound in the simplest way.
A molecular formula represents the formula of a compound as it exists. (can be reduced by a common factor)
Empirical : CH, Molecular: C6H6

75
Q

How do we find the empirical formula?

A

Since we will be given 2 percent compositions for different elements,we will be doing the steps for each element.

  1. turn percent composition into grams (no conversion)
  2. Convert grams into moles
  3. Once you have moles for both elements, divide each calculation by the smallest mole value in order to get a ratio.
  4. If your ratio is not a whole number, multiply by either 2,3,4 depending on the decimal. Once you have a whole number, go back to the elements and add their ratios as subscripts.
76
Q

How do we find molecular formula?

A

Since we will be given a Molar mass, we have to see if it will be true.

  1. Find empirical formula
  2. If values do not match, we can assume the formula was simplified and NOT the true molecular formula.
  3. We will then divide (molar mass molecular aka given)/ (molar mass calculated from empirical)
  4. once you get that value, it will let us know our empirical formula is off by a factor of it.
77
Q

What is the oxidation number of free elements?

A

0

78
Q

What is the oxidation of group 1 metals

A

+1

79
Q

What is the oxidation of fluorine in compounds?

A

-1

80
Q

What is the oxidation of group 2 metals?

A

+2

81
Q

What is the oxidation of group 3 ions?

A

+3

82
Q

What is the oxidation of hydrogen in compounds?

A

+1

83
Q

What is the oxidation of oxygen in compounds?

A

-2

84
Q

Oxidation is the ____ of electrons while Reduction is the _____ of electrons

A

Oxidation is the loss of electrons while Reduction is the gain of electrons (OILRIG)

85
Q

What is a reducing and oxidizing agent?

A

If we have an element that is oxidized, we have a reducing agent. If we have an element reduced, we have an oxidizing agent

86
Q

What are the four variables used to describe gas behavior?

A 
P: pressure in atm or torr (760 torr = 1 atm) 
T: temperature in Kelvin 
V: volume in liters
n: number of moles 
R: constant (0.0821)
87
Q

What is the ideal gas law?

A

PV = nRT

88
Q

What is STP (standard temp and pressure)

A

T: 273 K
P: 1 atm

89
Q

Why is 22.4 L an important value?

A

Because since all gases occupy the same volume at the same temperature and pressure, we can assume that one mole of any gas at STP has a volume of 22.4 L

90
Q

What is Boyles Law?

A

It tells us the relationship between volume and pressure (moles and temperature are constant)
As Volume increases, pressure decreases
P1V1= P2V2

91
Q

What is Charles law?

A

It is the relationship between Temperature and volume
As volume decreases, temperature decreases
V1/T1 = V2/T2

92
Q

What is Gay Lussac’s Law?

A

It is the relationship between pressure and temperature
As pressure increases, temperature increases
P1/T1 = P2/T2

93
Q

What is Avogadros law?

A

It is the relationship between moles and volume
As volume increases, moles increases
V1/n1 = V2/n2

94
Q

What is partial pressure?

A

Since gases exist in mixtures, we can identify the gas amounts for each individual element. According to Daltons Law of Partial Pressure, the total pressure is equal to the sum of all of the individual pressures

95
Q

What is henrys law?

A

(volume dissolved/volume of solvent) / gas pressure = (ml of gas/solvent) / atm

96
Q

As temperature decreases, solubility of gas

A

decreases

97
Q

As pressure increases, solubility of gas

A

increases

98
Q

Going from gas to solid is _______.Solid to Gas is

A

Sublimation, Deposition

99
Q

Changes of state are what type of reaction?

A

Physical

100
Q

Which is weaker IMF or chemical bonds?

A

Intermolecular forces

101
Q

What are the 3 types of IMF?

A

London Dispersion, Dipole Dipole, Hydrogen Bonds

102
Q

What is London Dispersion?

A

An attraction that is temporary and present in all molecules

103
Q

What is Dipole-Dipole?

A

A permanent attraction in polar molecules

104
Q

What is Hydrogen Bonding?

A

A Strong force that occurs when H bonds to either F,O or N

105
Q

How does IMF relate to energy needed for phase changes?

A

Strong IMF increase energy needed for phase change

106
Q

How does IMF relate to surface tension?

A

Strong IMF increases the surface tension

107
Q

How does IMF relate to vapor pressure?

A

Strong IMF decreases the vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure

108
Q

What is a vapor?

A

When a substance is present as both a gas and a liquid, the gas is a vapor. There is equilibrium between gas and liquid since it is in a closed space

109
Q

What is evaporation?

A

It is the same as vapor but it occurs in an open system and there is no equilibrium since particle are completely escaping

110
Q

When does boiling occur? evaporation?

A

When vapor pressure equal atmospheric pressure.When vapor pressure is less than atmospheric pressure, evaporation occurs

111
Q

In lower pressure, boiling points are

A

lower

112
Q

In higher pressure, boiling points are

A

higher

113
Q

What is the relationship between solids and melting points

A

The stronger the force, the higher the melting point. Covalent crystals have the highest, Ionic have an intermediate melting point and Molecular crystals (such as Ice) have a very low melting point

114
Q

When are solutions likely to form?

A

When 2 substances have similar IMF (except for substances that are only LDF)

115
Q

What is the difference between a solute and solvent?

A

A solute is the thing that gets dissolved, a solvent is the thing that solute dissolves in.

116
Q

A true solution is a _________ mixture

A

homogeneous

117
Q

What happens if a solution is saturated?

A

No more can dissolve

118
Q

What is the relationship between temperature and solubility?

A

As T increases, S increases

119
Q

Which solutions are generally soluble?

A

Group 1 metals, NH4 + salts, Nitrates, acetates, Sulfates are soluble except when combined with Ca, Sr or Ba

120
Q

Which solutions are generally insoluble?

A

Hydroxides except when combined with g1 metals or Sr, Ba

Phosphates and carbonates are insoluble except when combined with g1 metals

121
Q

If we have a displacement reaction, how do we find out the products of an equation?

A

They simply switch partners (metal first, nonmetal second). Make sure they are still balanced

122
Q

What is a complete ionic formula?

A

In this type of formula, anything that is aqueous, is written as individual ions. If it is a solid or liquid, they are written as wholes

123
Q

What is a Net ionic formula?

A

To generate a net ionic formula, we need to look at the complete ionic and make only write the things that changed.

124
Q

How do we solve for solution concentration?

A

concentration = amount of solute/ amount of solvent

125
Q

How do we calculate osmotic pressure?

A

i (n/v)

126
Q

When we have 2 substances with different concentrations and a semipermeable membrane, where will the solvent go towards?

A

The solution with the highest concentration

127
Q

What is a hypotonic cell?

A

When there is a low concentraion outside the cell so water moves in (blows up)

128
Q

What is a hypertonic cell?

A

When there is a high concentration outside the cell so water moves out (shrinks)

129
Q

When looking at an activation energy diagram, what comes first?

A

Reactants

130
Q

The Activation Energy (Ea) reaches which line?

A

Up to the reactants

131
Q

How do we calculate reaction rates?

A

(appearance of product) / time
OR
(disappearance of reactant) / time

132
Q

How does a catalyst affect the diagram?

A

It only changes the shape of the activation energy diagram since Ea is lowered

133
Q

How are catalysts identified given 2 reactions?

A

If an element is first a reactant and then a product, it will be a catalyst

134
Q

How are intermediates identified?

A

It is first a product, then a reactant

135
Q

What should we not include in the overall reaction?

A

catalysts or intermediates

136
Q

How do we calculate Keq? What are the units?

A

Keq = products/reactants In units of molarity

137
Q

Are all substances listed in Keq?

A

NO, only gases and aqueous solutions

138
Q

How do we find Keq between 2 sequences?

A

Mutliply them together

139
Q

What does LeChatliers principle tell us?

A

Our reaction shifts to the side that has less

140
Q

Does a catalyst increase or decrease the energy of an intermediate?

A

decrease

141
Q

Given H+, how do we solve for pH?

A

take the - log

142
Q

Given pH, how do we solve for pOH?

A

If we are given pH, simply use 14=pH + pOH and solve for pOH

143
Q

How do we solve for OH- concentration given H+?

A

Use the Kw formula Kw = H+ * OH-

144
Q

When asked to write a titration formula, what do we do?

A

You will be given an acid and base which will have to form a salt and water.

145
Q

How do we solve for titrations?

A

We will have to set up our conversions. Since we will be given volume of acid, make sure it is in liters and start off with that. Once you do, convert the liters into moles using molarity. After you have moles, convert into the bases moles using coefficients from the balanced equation. After you get moles of your base, divide by the volume given in the problem.

146
Q

In a dilution, what is constant? what changes?

A

In a dilution, concentration is reduced and amount of solute is constant

147
Q

What does a large Keq tell us about the reaction?

A

In a large Keq (greater than one), we can assume that products are favored, it is a favorable reaction

148
Q

What does a small Keq tell us about the reaction?

A

In a small Keq (less than one), we can assume that reactants are favored and it is an unfavorable reaction.

149
Q

How does heat relate to LeChatlier’s Principle?

A

If we have an endothermic reaction, heat is a reactant and it will shift right. If we have an exothermic reaction, heat is a product and it will shift left

150
Q

What are the 6 strong acids?

A

HCl, H2SO4, HI, HNO3, HBr, HClO4

151
Q

What makes an acid strong? weak?

A

Complete dissociation in solution means an acid is strong. A weak acid has a partial dissociation in solution.

152
Q

What is generally a weak acid?

A

Carboxyllic Acids

153
Q

What bases are strong?

A

Generally strong bases are metal hydroxides

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2

154
Q

How do we tell the difference between Ka and Kb?

A 
Ka= acid + water ⇌ H3O + conjugate base 
Kb= base+ water ⇌ OH- + conjugate acid
155
Q

How does the K value relate to favoritism?

A

If we have two values with a small Ka Value, the one that is the biggest (even though they both favor reactants) is the stronger weak (acid/base).

156
Q

How does the K value relate to an inverse relationship in strength of weak acids/bases?

A

If we determine we have a weak acid, we know the conjugate base will be strong. If we have a weak base, the conjugate acid will be strong.

157
Q

When calculating concentration of H3O+ or OH-, what will determine acidic or basic?

A

If we have a higher H3O + concentration, it is acidic. If OH- is higher, it is basic

158
Q

When does a buffer work at its best?

A

When ph = pKa

159
Q

To find concentration of H3O+, given pH what do we do?

A

10 ^-pH (antilog of pH)

160
Q

To find concentration of OH-, given pOHwhat do we do?

A

10 ^-pOH (antilog of pOH)

161
Q

How do we find the sequences of polyprotic acids?

A

In the 1st step, we will have an acid + water = Hydronium and base (H+ when to water and created H3O+)
In the second step, our base will be our acid and we will have acid + water = Hydronium + base ( one less H+)

162
Q

How do we calculate pH given molarity for acid base and Ka?

A

Use the pKa + log (base/acid) formula

163
Q

What happens in alpha decay?

A

Atomic # decreases by 2

Mass # decreases by 4

164
Q

What happens in Beta Decay?

A

Atomic # increases by 1

Mass # stays the same

165
Q

What happens in positron decay?

A

Atomic # decreases by 1

Mass # stays the same

166
Q

In a pH scale, what values indicate an acidic solution? basic?

A

In a pH scale, acidic is anything less than 7 and basic is anything greater than 7

167
Q

In a pOH scale, what values indicate an acidic solution?

A

In a pOH scale, acidic is anything greater than 7, basic is anything less than 7

168
Q

If we are given Ka, how do we solve for pKa?

A

-log

169
Q

If we are given pKa, how do we solve for Ka?

A

10^-pKa

Chemistry 100 SDSU (5 decks)

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