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Final study Guide Flashcards

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0
Q
  • the oxidation number of atoms in a compound must equal zero
  • the sum of the oxidation number in polyatomic ions is zero
  • alkali metals have the oxidation number +1.
  • an ions charge is equals to its oxidation number

Which one isn’t true.

A

The sum of the oxidation number in polyatomic ions is zero

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1
Q

What is a compound that contains a water molecule in its crystalline structure?

A

Hydrates

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2
Q

The Greek prefixes system is normally used for either ionic or covalent compounds. T/F

A

False

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3
Q

What is a compound that contains hydrogen, oxygen, and another nonmental?

A

Ternary acid

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4
Q

What is the oxidation number of H in MgH2.

A

-1

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5
Q

The prefix hepta- means

A

7

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6
Q

Name the following compound: P2O5

A

Diphosphorous pentoxide

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7
Q

Write a chemical formula for the following compound: ammonium fluoride

A

NH4F

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8
Q

What represents the number of electrons that an atom in a compound must gain or lose to return to its neutral state?

A

Oxidation number

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9
Q

What is the oxidation number of Cu in CuSO4?

A

+2

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10
Q

System for naming compounds

A

Nomenclature

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11
Q

Another name for stock system which indicates the oxidation number used of the metal in the ionic compound

A

Roman numeral system

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12
Q

Covalently bonded groups of atoms that carry a charge

A

Polyatomic atoms

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13
Q

The number of electrons that an atom in a compound must gain or lose to return to its neutral state

A

Oxidation number

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14
Q

A compound that is not ionic or an acid

A

Binary covalent compound

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15
Q

Acids consisting of hydrogen and one other nonmetal

A

Binary acid

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16
Q

Anions that contain oxygen and one other element

A

Oxyanions

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17
Q

Indication of how many atoms of each element are in a binary covalent compound

A

Greek prefix system

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18
Q

The more electronegative element receives a negative oxidation number, and a less electronegative element receives a positive oxidation number. T/F

A

False

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19
Q

The sum of the oxidation number of all the atoms in a compound must equal zero. T/F

A

True

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20
Q

Group one has what oxidation number?

A

+1

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21
Q

What is the oxidation number of halogens typically have when they bond with metals?

A

-1

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22
Q

What is the oxidation number of P in Cu3P2?

A

-3

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23
Q

What is the oxidation number of Hg3(PO4)2?

A

+2

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24
Q

Identify the name for the following compound: Pb(NO3)2

A

Lead (II) nitrate

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25
Q

Identify the name for the following compounds: KClO3

A

Potassium Chlorate

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26
Q

Identify the name for the following compounds: MgSO4 x 7H2O

A

magnesium sulfate heptahydrate

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27
Q

Write the correct chemical formula for the following compound: potassium cynide

A

KCN

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28
Q

Write the correct chemical formula for the following compound: aluminum phosphate

A

AlPO4

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29
Q

Write the correct chemical formula for the following compound: ammonium fluoride

A

NH4F

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30
Q

Write the correct chemical formula for the following compound: sodium phosphate

A

Na3PO4

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31
Q

Write the correct chemical formula for the following compound: aluminum and chlorine

A

AlCl3

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32
Q

Write the correct chemical formula for the following compound: potassium and oxygen

A

K2O

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33
Q

Write the correct chemical formula for the following compound: hydrogen and bromine

A

HBr

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34
Q

Briefly describe 3 of the 5 oxidation rules.

A

The second rule is the ion chare rule. This rule states that the oxidation number of an element is formed by its charge. For example, halogens main charge is -1 because they only need to gain one electron to be happy, so it is -1 when it is bonded with a normal metal. The third rule is the zero sum rule. This rule states that the oxidation numbers in a compound must come together to form zero. The fourth rule states that there is almost a mini pattern of oxidation numbers. Group 1 elements have the oxidation number of +1. Alkaline earth metals have the oxidation number +2. Oxygens main oxidation number is -2, unless it is bonded with flourine which then it’s oxidation number is -1. And halogens, when bonded with a metal have an oxidation number of -1.

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35
Q

An expression that represents a chemical reaction by using chemical formulas, chemical symbols, and coefficients

A

Chemical equation

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36
Q

Substances present before a chemical reaction

A

Reactants

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37
Q

Substances present after a chemical reactions

A

Products

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38
Q

Chemical equation that follow the law of mass conservations (equal substances on both sides of the equation)

A

Balanced equation

39
Q

Tells how many atoms, ions, molecules, or formula units are present in a chemical equation

A

Coefficients

40
Q

Reactions that occur both forward and in reverse

A

Reversible reactions

41
Q

Arrangement of metals in order of the activity

A

Activity series

42
Q

Substances that appear in the reactions and products that remain unchanged

A

Spectator ions

43
Q
  • Identifies all substances involved in a reaction
  • Shows the composition of the substances involved
  • Indicates the mass of products and reactants
  • Accounts for all atoms involved in the reaction

Which of the following does not represent a function of a balanced equation?

A

Indicates the mass of products and reactants

44
Q

An equation may be balanced by adjusting the coefficients or the subscripts. T/F

A

False

45
Q

Identify the following reaction that is occurring: 4Fe + 3O2 –> 2Fe2O3

A

Synthesis is reaction

46
Q

Identify the following reaction that is occurring:

2AlCl3 –> 2Al + 3Cl2

A

Decomposition reaction

47
Q

Identify the following reaction that is occurring:

2NaCl + H2SO4 -> Na2SO4 + HCl

A

Double replacement reaction

48
Q

Identify the following reaction that is occurring:

TiCl4 + 4Na -> Ti + 4NaCl

A

Single replacement reaction

49
Q

Identify the following reaction that is occurring:

Mg(OH)2 + 2HNO3 -> Mg(NO3)2 + 2H2O

A

Double replacement reaction

50
Q

Identify the following reaction that is occurring:

NH3 + CO2 + H2O -> NH4HCO3

A

Synthesis reaction

51
Q

Indicates a gaseous product

A

(g)

52
Q

Indicates the substance is dissolved in water

A

(aq)

53
Q

Indicates a solid reaction

A

(s)

54
Q

Means yield or produces

A

—->

55
Q

Indicates a liquid reactant or product

A

(l)

56
Q

The solid that falls out of a solution

A

Precipitate

57
Q

What is the only thing you are allowed to change when balancing an equation?

A

Coefficients

58
Q

When looking at an activity series, the higher up an element is, the more reactive it is. T/F

A

True

59
Q

Formula that shows the type of atoms involved, the exact composition of each molecule, and the arrangement of chemical bonds

A

Structural formula

60
Q

The mass of one mole of any pure substance

A

Molar mass

61
Q

Formula that tells what elements are present and give the simplistic whole number ratio of atoms in the compound

A

Empirical formula

62
Q

The coefficients from the balanced equations give the rations retween the moles of one substance

A

Mole ratios

63
Q

The ratio of elements in a compound is constant for every particle in that compound

A

Law of definite composition

64
Q

One mole is equal to avegadro’s number. T/F

A

True

65
Q

What is the mathematical relationship between the amounts of reactants and products in a chemical reaction?

A

Stoichiometry

66
Q

What is used up before the other reactants?

A

Limiting reactants

67
Q

What is the measured around of products at thee d of a reaction?

A

Actual yield

68
Q

What is the maximum amount of products that could be created from a given amount of reactants?

A

Theoretical yield

69
Q

The number of helium is equal to the number of lead atoms Ina mole of lead. T/F

A

True

70
Q

Shows the type and numbers of atoms involved as they appear in the molecule

A

Molecular formula

71
Q

A mole of sucrose has the same mass as a mole of water molecules. T/F

A

False

72
Q

A molecular compound may have identical empirical and molecular formulas. T/F

A

True

73
Q

The mole must be used to quantify both large objects as well small objects. T/F

A

False

74
Q

Conversions from gram to moles

A

amu

75
Q

Conversion from mole to mole

A

Molar ratio

76
Q

Conversion from moles to number of particles

A

Avegadro’s number

77
Q

A gas easily mingles with another porous substance

A

Permeability

78
Q

High pressure can squeeze into smaller volumes

A

Compressibility

79
Q

A gas moves through a tiny opening into an evacuated chamber

A

Effusion

80
Q

Collisions of gas molecules conserve energy

A

Elasticity

81
Q

A gas quickly expands to fill a low pressure region

A

Expansibility

82
Q

Gas molecules move constantly to uniformly fill their container

A

Diffusion

83
Q

Diffusion could not occur if molecules were not in constant motion. T/F

A

True

84
Q
  • gas particles move randomly and rapidly
  • gas particles lose energy when they collie with one another
  • gas particles are separated by great distances
  • gas particles do not interact with each other except during momentary collisions

Which one is not a prediction of the kinetic- molecular theory?

A

Gas particles lose energy when they collide with one another

85
Q

Which gas law focuses on the relationship between pressure and volume?

A

Boyles law

86
Q

Which property of gases best explains why spooked meat in a sealed plastic container eventually makes a refrigerator smell?

A

Permeability

87
Q

Gases temperatures must be measured in Celsius temperatures. T/F

A

False

88
Q

The gas law that focuses on the relationship between volume and temperature is

A

Charles law

89
Q

If you are collecting gas by water displacement, you must Renee to adjust for

A

Vapor pressure

90
Q

Collisions constantly change the speed and direction of gas molecules. T/F

A

True

91
Q

What pair is related by an inverse relationship?

A

Volume and pressure

92
Q

All gas molecules of the same type have the same speed at the same temperature. T/F

A

False

93
Q

The SI unit for pressure is the pascal. T/F

A

True

94
Q

The abbreviation STP represents the standard condition of 760 ATM and 273 K. T/F

A

False

95
Q

Depends on the force and number of collisions per second

A

Pressure

96
Q

Determined on the average kinetic energy of molecules

A

Temperature

Chemistry (4 decks)

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