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Gen Chemistry 1 > Gen Chem Exam 2 > Flashcards

Gen Chem Exam 2 Flashcards

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1
Q

How many grams are in 1 kg?

A

1000 grams

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2
Q

How many cm are in 1 m?

A

100 cm

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3
Q

How many mL are in 1 L?

A

1000 mL

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4
Q

Are numbers that are not 0 considered significant?

A

Yes

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5
Q

Is the number at the beginning of a decimal considered significant?

A

No

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6
Q

Is the zero between nonzero digits considered significant?

A

Yes

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7
Q

Is the zero at the end of a decimal considered significant?

A

Yes

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8
Q

Are the zeros in large numbers that are used as a placeholder considered significant?

A

No

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9
Q

Are the numbers written out in standard notation considered significant?

A

Yes

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10
Q

How many sig figs are in 122.45?

A

5

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11
Q

How many sig figs are in 205?

A

3

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12
Q

How many sig figs are in 16.00?

A

4

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13
Q

How many sig figs are in 5.70 x 10^3?

A

3

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14
Q

How many sig figs are in 0.075?

A

2

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15
Q

How many sig figs are in 850,000?

A

2

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16
Q

What are exact numbers?

A

Numbers that are not measured and are obtained by counting.

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17
Q

What are exact numbers used for?

A

In definitions to compare two units
- same measuring system

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18
Q

Rounding a number ___ the level of precision.

A

Decreases

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19
Q

How do you determine the amount of sig figs when multiplying/dividing?

A

Use the lowest number of sig figs of a number in the equation.

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20
Q

6.0 x 2.00 =

A

12 (2 sig figs)

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21
Q

How do you determine the amount of sig figs when adding/subtracting?

A

Use the same number of decimal places as the number with the fewest decimal places.

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22
Q

65.09 - 3.0 =

A

62.1 (1 decimal place)

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23
Q

What are the most commonly used prefixes for displaying LARGER numbers?

A
  1. Kilo
  2. Mega
  3. Giga
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24
Q

What are the most commonly used prefixes for displaying SMALLER numbers?

A
  1. Centi
  2. Milli
  3. Micro
  4. Nano
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25
Q

Cubic Centimeter (cc)

A

The volume of a cube whose dimensions are 1 cm on each side.

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26
Q

The cubic centimeter has the same volume as a ___.

A

Millimeter

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27
Q

Equalities

A

Use two different units to describe the same measured amount.

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28
Q

Can any equality be written as a conversion factor?

A

Yes

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29
Q

How many centimeters are in 1 inch?

A

2.54 cm

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30
Q

Density

A

Compares the mass of an object to its volume.

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31
Q

What is the formula for density?

A

mass/volume

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32
Q

Volume

A

The amount of space a substance occupies.

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33
Q

Mass

A

A measure of the quantity of material an object contains.

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34
Q

What are metric units used for measuring?

A
  1. Length
  2. Mass
  3. Volume
  4. Temperature
  5. Time
    (everything basically)
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35
Q

Chemical Bonds

A

Formed when atoms gain, lose, or share valence electrons to acquire 8 valence electrons.

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36
Q

Noble Gas Configuration

A

8 valence electrons

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37
Q

Octet Rule

A

Atoms lose/gain electrons to have 8 valence electrons?

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38
Q

Ionic Bonds

A

Metals lose valence electrons and are transferred to a nonmetal.

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39
Q

Ionic Bonds turn into…

A

Ionic Compounds

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40
Q

Covalent Bonds

A

Nonmetals share electrons to attain a noble gas configuration.

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41
Q

Covalent Bonds turn into…

A

Molecular Compounds

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42
Q

Cations

A

Positively charged ions created by the loss of electrons

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43
Q

Anions

A

Negatively charged ions created by the gain of electrons.

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44
Q

Positive Ions

A

Metals lose electrons

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45
Q

Negative Ions

A

Nonmetals gain electrons

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46
Q

Ionic Compounds

A

Positive and negative charges held together by the strong electrical attractions between oppositely charged ions.

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47
Q

What are the 2 properties of ionic compounds?

A
  1. High melting points
  2. Solids at room temperature
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48
Q

Chemical Formula

A

Symbols and subscripts written in the lowest whole-number ration of the atoms/ions.

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49
Q

Formula Unit

A

The lowest whole number combination for the compound.

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50
Q

What does the sum of ion charges in a chemical formula equal?

A

0

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51
Q

How do you name an ionic compound?

A
  1. Write the full name of the metal
  2. Write the first syllable of the non metal
  3. Add “-ide” to the end of the non metal.
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52
Q

What can be placed after the name of an ion to reveal it’s charge?

A

Roman numeral

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53
Q

How do you find the ion charges in groups 1A and 2A?

A

Add a positive after the group number.

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54
Q

How do you find the ion charges in groups 5A, 6A, and 7A?

A
  1. 8 - (group number)
  2. Add a negative after
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55
Q

Name the ionic compound.
SnO2

A

Tin (IV) Oxide

56
Q

What are the steps to writing formulas for compounds containing polyatomic ions?

A
  1. Identify cation and polyatomic ion (anion)
  2. Balance the charges using the criss cross method.
  3. Write the formula using the cation first, as well as their subscripts
57
Q

How do you name ionic compounds with polyatomic ions?

A
  1. Write the name of the polyatomic ion (metal).
  2. Write the name of the polyatomic ion.
58
Q

What is the simplest molecule?

A

H2

59
Q

What type of bond is H2?

A

Covalent bond

60
Q

Double Bond

A

Atoms share two pairs of electrons.

61
Q

Triple Bond

A

Atoms share three pairs of electrons.

62
Q

When do double and triple bonds form?

A

When there are not enough electrons to complete the octet.

63
Q

What are the 3 exceptions to the octet rule?

A
  1. Hydrogen requires only 2 electrons to form a noble gas arrangement.
  2. Boron requires 6 electrons, which only makes 3 bonds.
  3. Beryllium requires 4 electrons, which only makes 2 bonds.
64
Q

Electronegativity (EN)

A

An atoms ability to attract the shared electrons in a bond.

65
Q

What does the higher value of electronegativity mean?

A

A greater ability to attract electrons.

66
Q

Is there a scale of electronegativity?

A

There is a relative scale with no units.

67
Q

What are the periodic trends of electronegativity?

A
  • Increases from left to right
    -Increases from top to bottom
    -High for nonmetals
    -Low for metals
68
Q

How do you predict the polarity of a bond?

A

The difference in electronegativity of bonding atoms.

69
Q

Nonpolar Bond

A

Electrons are shared equally

70
Q

Polar Bond

A

Electrons are shared unequally

71
Q

What is the EN value range for nonpolar covalent bonds?

A

0-0.4

72
Q

What is the EN value range for polar covalent bonds?

A

0.5-1.8

73
Q

What is the EN value range for ionic bonds?

A

1.9 +

74
Q

Dipole

A

Seperation of charges in a polar bond.

75
Q

What symbol is used to distinguish the dipole charges?

A

g (delta)

76
Q

Which element has a + g and which one has a -g?

A
  • Larger EN element has the -g
    -Smaller EN element has the +g
77
Q

What type of elements do ionic bonds form between?

A

metal and nonmetal ions

78
Q

What does it mean when a molecule is blue on one end and red on the other?

A

The molecule is polar

79
Q

What does it mean when a molecule is all green?

A

The molecule is non-polar

80
Q

In what two situations do non-polar molecules arise?

A
  1. The molecule contains all non polar bonds (H2, Cl2, or CH4) and no lone pairs on the central atom.
  2. The molecule contains polar bonds, but the polar bonds cancel in a symmetrical arrangement.
81
Q

What are the three non polar molecules?

A
  1. H2
  2. Cl2
  3. CH4
82
Q

Why are polar molecules polar?

A
  1. The electrons are shared unequally
    AND/OR
  2. The polar bonds in the molecule do not cancel each other
83
Q

Do single dipoles cancel?

A

No

84
Q

In gases, molecules are ___ from each other.

A

Far

85
Q

In liquids and solids, the molecules are ___ to each other.

A

close

86
Q

Ion Dipole Interactions

A

Relatively strong electrostatic attractions between ions and polar molecules
-cause the dissolution of ionic solids in polar solvents such as water.

87
Q

Dipole Dipole Interactions

A

Attractive forces between polar molecules.

88
Q

Hydrogen Bond

A

Hydrogen bonded to F, O or N.
- VERY STRONG bond
- Type of dipole dipole interaction

89
Q

Dispersion Forces

A

Weak attractions that can occur between two molecules.

90
Q

What causes dispersion forces?

A

Temporary dipoles that develop when molecules bump into each other.

91
Q

What do dispersion forces make possible?

A

Non polar molecules to form liquids and solids.

92
Q

What types of molecules have dispersion forces?

A

ALL MOLECULES

93
Q

What type of force is stronger: Intramolecular or Intermolecular?

A

INTRAmolecular

94
Q

What types of bonds are INTRAmolecular bonds?

A
  1. Ionic Bond
  2. Covalent Bond
95
Q

What types of bonds are INTERmolecular bonds?

A
  1. Hydrogen Bond
  2. Dipole-Dipole Interaction
  3. Dispersion Forces
96
Q

What is an example of a dispersion force?

A

O2, F2, etc.

97
Q

What is an example of hydrogen bonding?

A

H2O

98
Q

What is an example of Dipole-Dipole Attractions?

A

CH2O

99
Q

Strong forces have a ___ melting/boiling point.

A

Higher

100
Q

Chemical Change

A

A substance is converted
into one or more substances with different
formulas and different properties.

101
Q

What are the 4 possible observations of a chemical change?

A
  1. Formation of bubbles
  2. Color change
  3. Production of a solid
  4. Heat produced or absorbed
102
Q

What size of a chemical equation do reactants go on?

A

Left

103
Q

What side of a chemical equation do products go on?

A

Right

104
Q

What two factors help identify a balanced equation?

A
  1. No atoms are lost or created
  2. The number of atoms on the reactant side is equal to the number of atoms of the same element on the product side.
105
Q

Law of Conservation of Matter

A
  1. Matter cannot be created or destroyed
  2. No change in total mass occurs
  3. The mass of products is equal to the mass of reactants
106
Q

Avogadros Number

A

6.02 x 10^23 items

107
Q

The mole is a ___ term.

A

counting

108
Q

1 mole contains ____ worth of items.

A

avogadro’s number

109
Q

What do the subscripts in a formula represent?

A
  1. The relationship of atoms in the formula.
  2. The moles of each element in 1 mole of compound.
110
Q

How many moles of each element are in C9 H8 O4?

A
  1. C= 9 moles
  2. H = 8 moles
  3. O = 4 moles
111
Q

What is the molar mass of an element used to convert?

A
  1. moles of an element to grams
  2. grams of an element to moles
112
Q

How do you convert from grams of an element/compound to moles?

A

Using the molar mass (g/mole)

113
Q

How do you convert from atoms to moles of an element?

A

Avogadros number

114
Q

How do you convert from moles of an element to moles of a compound?

A

Formula Subscripts

115
Q

How do you convert from molecules to moles of a compound?

A

Avogadros number

116
Q

What are the 5 types of chemical reactions?

A
  1. Combination (synthesis)
  2. Decomposition
  3. Single Replacement
  4. Double Replacement
  5. Combustion
117
Q

Can chemical reactions fit into more than one type of reaction?

A

Yes

118
Q

Combination (Synthesis) Reaction

A
  • Two or more elements form one product
  • Simple compounds combine to form one product
119
Q

Decomposition Reaction

A

One substance splits into two or more simpler substances

120
Q

Single Replacement Reaction

A

One element takes the place of a different element in another reacting compound

121
Q

Double Replacement Reaction

A

Both ions in the reactant compounds switch places.

122
Q

Combustion Reaction

A
  • A carbon-hydrogen containing compound burns in oxygen gas to form CO2 and H2O
  • Energy is released as a product in the form of heat.
123
Q

What type of chemical reaction is…
2Mg + O2 –> 2MgO

A

Combination (synthesis)

124
Q

What type of chemical reaction is…
2HgO –> 2 Hg + O2

A

Decomposition

125
Q

What type of chemical reaction is…
Zn + 2HCl –> ZnCl2

A

Single Replacement

126
Q

What type of chemical reaction is…
AgNO3 + NaCl –> AgCl + NaNO3

A

Double Replacement

127
Q

What type of chemical reaction is…
CH4 + 2O2 –> CO2 + 2H2O + energy

A

Combustion

128
Q

How is carbon monoxide (CO) produced?

A

When oxygen supply is limited, an incomplete combustion from burning gas, oil or wood occurs

129
Q

Why is CO toxic?

A

It binds to the hemoglobin in your blood and blocks oxygen from binding.

130
Q

What is needed when burning fuels?

A

Good ventilation

131
Q

What is happening to electrons when rust forms?

A

The electrons are transferring from one substance to another.

132
Q

Oxidation Reduction Reactions

A

Electrons are transferred from one substance to another.

133
Q

What can oxidation not occur without?

A

Reduction

134
Q

“OIL RIG”

A

Oxidation
Is
Loss of electrons

Reduction
Is
Gain of electrons

135
Q

What type of reaction is this…
Cu –> Cu2+ + 2e

A

Oxidation Reduction

Gen Chemistry 1 (10 decks)

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