Chemistry Final

Front 1

Chemistry is the study of ______

Back 1

of all substances and changes that they undergo

Front 2

In Chemistry, the ___ is used

Back 2

International System of Units, SI

Front 3

Which of the following would be used to convert units?

Back 3

Dimensional analysis

Front 4

Which of the following states that in any process, energy is neither created nor destroyed?

Back 4

Law of conservation of energy

Front 5

The lowest temperature theoretically possible is called______.

Back 5

absolute zero

Front 6

Matter must have ______

Back 6

mass and volume

Front 7

There are ___ states of matter

Back 7

4

Front 8

Matter has _____.

Back 8

physical and chemical properties

Front 9

A(n) ___ cannot be changed into simpler substances by a chemical reaction

Back 9

element

Front 10

The proportions of the elements within a compound ________.

Back 10

never changes

Front 11

a mixture ______

Back 11

is a blend of two or more substances

Front 12

mixtures can be categorized as _____.

Back 12

homogeneous and heterogeneous

Front 13

The smallest particle of an element is the ______

Back 13

atom

Front 14

The electrical charge of an atom is____

Back 14

neutral

Front 15

Atoms are composed of ___

Back 15

electrons, protons, and neutrons

Front 16

an "atom" or group atoms having an electrical charge is a(n) ____.

Back 16

ion

Front 17

An ion always contains an ____.

Back 17

unequal number of protons and electrons

Front 18

Two atoms are isotopes is they contain___

Back 18

the same number of protons but different numbers of neutrons

Front 19

When electrons are in the lowest energy orbital available, the atom is ____.

Back 19

in the ground state

Front 20

According to the Bohr model, when an electron absorbs an appropriate amount of energy ___.

Back 20

the electron moves away from the nucleus a distance corresponding to the amount of energy absorbed by the electron

Front 21

Orbitals have characteristics shapes, size and energies (True or False)

Back 21

True

Front 22

The distribution of electrons amongst the Orbitals of an atoms is its

Back 22

electron configuration

Front 23

Elements in a ___ have similar properties

Back 23

group

Front 24

Metals can be found on the ___ side of the periodic table.

Back 24

left

Front 25

Metals are ___.

Back 25

lustrous ductile, malleable and good conductors of heat and electricity

Front 26

an atom which has gained two electrons has a charge of ___.

Back 26

-2

Front 27

ionic compounds are held together by ____.

Back 27

electrostatic attraction

Front 28

What name is given to a positively charges ion?

Back 28

cation

Front 29

The ___ rule states that toms tend to gain, lose or share electrons in order to acquire a full set of valence electrons

Back 29

octet

Front 30

Ionic compounds are written with ____.

Back 30

an empirical formula

Front 31

the smallest unit of a molecular compound having all the properties of the compound is a(n) _____.

Back 31

molecule

Front 32

A ___ formula depicts the arrangement of the atoms within a molecule

Back 32

structural

Front 33

Lewis dot structures show ____.

Back 33

only electrons in the outermost energy level

Front 34

In a Lewis dot structure of molecular compounds a single dash represents ____.

Back 34

a shared pair of electrons

Front 35

In a polar bond ____.

Back 35

electrons are not shared equally

Front 36

To form a covalent bond, atoms share

Back 36

valence electrons

Front 37

The formula CuSO4 * 5H2O indicates____.

Back 37

the substance is only capable of dissolving in water

Front 38

In the compound Ca3(PO4)2, there are ___ oxygen atoms.

Back 38

eight

Front 39

Prefixes are use in ____ compounds to indicate the number of atoms in the compound

Back 39

molecular

Front 40

The physical states of nearly all ionic compounds at room temperature is ___.

Back 40

liquid

Front 41

How does a covalent bond differ from an ionic bond?

Back 41

An ionic bond is the transfer of electrons and a covalent bond is the sharing of electrons

Front 42

-NO3^-1 is a ___ ion

Back 42

nitrate

Front 43

-SO4^-2 is a ___ ion

Back 43

sulfate

Front 44

Which of the following is the formula for hydrochloric acid?

Back 44

HCl

Front 45

Which of the following is the formula for sulfuric acid?

Back 45

H2SO4

Front 46

Which of the following is true of a chemical reaction?

Back 46

New substances must form

Front 47

A substance that enters into a chemical reaction is called a ___.

Back 47

reactant

Front 48

A substance that is formed by a chemical reaction is called a ___.

Back 48

product

Front 49

In a chemical equation, the symbol that takes the place of the words "reacts with" is a(n) _____.

Back 49

plus sign

Front 50

In a chemical equation, the symbol that takes the place of the word "yields" is a(n) ____.

Back 50

arrow

Front 51

In a chemical reaction, what is the relationship between the total mass of the reactants and the total mass of the products?

Back 51

They must be equal

Front 52

In a chemical equation, the number of molecules of a given substance is indicated by a ___.

Back 52

coefficient

Front 53

How many atoms of oxygen are represented in 2Ca(NO3)2?

Back 53

12

Front 54

The sum of the atomic masses of all atoms in a compound is called the ____.

Back 54

Formula mass

Front 55

A mole of carbon dioxide contains 6.02 x 10^23 ___.

Back 55

molecules

Front 56

The molar mass of a compound depends upon the ____.

Back 56

mass of each element in the compound

Front 57

In chemistry, stoichiometry is the study of _____.

Back 57

the quantitative relationship that exists in chemical formulas and chemical reactions

Front 58

The amount of product formed in a chemical reaction is determined by the amount of the ____.

Back 58

limiting reactant

Front 59

Which of the following is NOT a property of gases?

Back 59

Gases are weightless near the surface of the earth

Front 60

In which of the following would the attractive force between particles be the smallest?

Back 60

gas

Front 61

In which of the following would the density of the substance be the greatest?

Back 61

solid

Front 62

Which of the following represents the strongest attractive force?

Back 62

ionic bond

Front 63

A covalent bond is an example of a ____.

Back 63

Intermolecular form

Front 64

In which of the following states of matter will diffusion be the most rapid?

Back 64

gas

Front 65

Liquid A and Liquid B have boiling points of 100°C and 75°C respectively. In which liquid is the attractive force between particles the strongest?

Back 65

A

Front 66

As the temperature of a liquid increases, the viscosity of the liquid ____.

Back 66

decreases

Front 67

The greater the surface tension of a liquid ___.

Back 67

the stronger the intramolecular forces

Front 68

___ have a highly ordered, repeating pattern.

Back 68

Crystalline solids

Front 69

Viscosity ____.

Back 69

is the resistance of a liquid in motion

Front 70

In condensation ____.

Back 70

a gas changes into a liquid

Front 71

When a liquid within a container evaporates ____.

Back 71

the escaping particles have sufficient kinetic energy to break the intermolecular forces of attraction

Front 72

As the temperature of a liquid increases the kinetic energy of the particles ____.

Back 72

increases

Front 73

As the temperature of a liquid increases the rate of evaporation ____.

Back 73

increases

Front 74

Isoproplyl alcohol (rubbing alcohol) evaporates more quickly at the same temperature than water because ____.

Back 74

Alcohol has smaller intermolecular forces

Front 75

You are traveling in the Himalayan Mountains for the summer. As you boil water to make meals you recognize it takes longer to cook meals. This is because ____.

Back 75

The water boils at a temperature below 100°C

Front 76

The temperature of the boiling water is 100°C at one atmosphere pressure, and the temperature of the steam above water is _____.

Back 76

Equal to 100°C

Front 77

The melting point of a solid is .1°C above the freezing point of the solid

Back 77

False

Front 78

Sublimation is the change of a ____.

Back 78

Solid to a gas

Front 79

The kinetic-molecular theory applies to ___.

Back 79

only gases

Front 80

The physical properties of gases, liquids and solids are derived from ____.

Back 80

The strength of attractive forces

Front 81

Which of the following terms represent opposite changes of state?

Back 81

Sublimation and deposition

Front 82

A liquid is a closed container. After a period of time, ______.

Back 82

A dynamic equilibrium is reached

Front 83

Substances which are volatile evaporate easily and _____.

Back 83

Have weak intermolecular forces

Front 84

All solutions have the following properties except ____.

Back 84

Solution particles do not separate or settle out.

Front 85

Two substances are miscible ____.

Back 85

If the two substances will mix in any proportions

Front 86

Solutions with water as the solvent are called ____.

Back 86

Aqueous solutions

Front 87

Molarity is expressed as ____.

Back 87

Moles of solute / liters of solvent

Front 88

A solution that contains as much solute as can possibly be dissolved under the existing conditions is _____.

Back 88

Saturated

Front 89

Which of the following's solubility is most affected by pressure?

Back 89

gases

Front 90

A bottle of pepsi has sat in the sun on a hot summer day. When the bottle was opened the gas/ soda vigorously shot from the bottle. Which of the following is an explanation for this event?

Back 90

The increased temperature made the gas less soluble

Front 91

A nonelectrolyte is dissolved into water. The solution formed ____.

Back 91

Will not conduct electricity

Front 92

You have a sugar/ water solution. If vigorously heated over a period of time and boiling is achieved, the boiling point of the sugar/ water solution will ____.

Back 92

Continue to increase with heating

Front 93

Grinding urea into small particles will allow the urea to dissolve faster in water if it weren't ground up. This is because ____.

Back 93

Grinding urea will increase the surface area.

Front 94

A volatile substance ____.

Back 94

evaporates quickly

Front 95

The addition of a non volatile solute will cause the boiling point of the solvent to ____.

Back 95

Increase

Front 96

Any chemical reaction in which the products can regenerate the reactants is called a(n) ____.

Back 96

reversible reaction

Front 97

What symbol is used to indicate a reversible reaction?

Back 97

<---->

Front 98

The process in which ions leave a solution and regenerate an ionic solid is called _____.

Back 98

precipitation

Front 99

How many ions will one formula unit of CaCl2 produce?

Back 99

3

Front 100

An aqueous solution is a solution in _____.

Back 100

water

Front 101

The symbol (aq) is used to denote a solution that is ____.

Back 101

Aqueous

Front 102

The characteristic taste of bases is best described as ____.

Back 102

bitter

Front 103

The reaction of acids with metal produces the gas ____.

Back 103

hydrogen

Front 104

Acids and bases are conductors of electricity, they are referred as ____.

Back 104

electrolytes

Front 105

Substances that change color when added to acids or bases are called ____.

Back 105

Indicators

Front 106

The relative strengths of acids are determined by the extent to which the acids particles ____.

Back 106

ionize in water solution

Front 107

H2SO4 is an acid. (True or False)

Back 107

True

Front 108

A solution with the pH of 8.1 is ____.

Back 108

a base

Front 109

What is the molar mass of NaHCO3?

Back 109

84 grams

Front 110

Find the molar mass of 0.159 moles of SiO2

Back 110

9.54 grams

Front 111

What is the percentage of nitrogen in ammonia (NH3)?

Back 111

82.3%

Front 112

What is the molarity of a a solution prepared by dissolving 1.1 moles of NaOH in enough water to make 1.2 liters of solution?

Back 112

.91 M

Front 113

What is the pH of a solution having an hydronium ion concentration of 5.02 x 10-12?

Back 113

11.3

Front 114

The pH of a solution is 3.5. What is the hydronium ion concentration of the solution?

Back 114

3.16 x 10-4

Front 115

Identify the reactants in the following equation: BaCl2 + Na2SO4 ---> BaSO4 + NaCl

Back 115

BaCl2 + Na2SO4

Front 116

Is the following equation balanced?

BaCl2 + Na2SO4 ---> BaSO4 + NaCl

Back 116

No

Front 117

What are the products in the following reaction? Mg + H2SO4 ---> ?

Back 117

MgSO4 + H2

Front 118

Write a word equation for the following chemical reaction: Mg(s) + HCl(aq) + H2(g)

Back 118

Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas

Front 119

Write a word equation for the following chemical reaction: KOH + FeCl3 ----> KCl + Fe(OH)3

Back 119

Potassium hydroxide reacts with iron III chloride to yield potassium chloride and iron III hydroxide

Front 120

The following reaction would be an example of a ____ reaction: KOH + FeCl3 ----> KCl + Fe(OH)3

Back 120

double replacement

Front 121

How many atoms are in 1.0 x 10^-3 moles of helium, He?

Back 121

6.0 x 10^20