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Chemisty > Unit 3 and 4 > Flashcards

Unit 3 and 4 Flashcards

1
Q

What did John Dalton do?

A
  • Determined atomic masses of elements
  • Found how elements combine to form compounds
  • Chemical formulas show characteristic proportions
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2
Q

The ratio of the two masses of one element that react with a given mass of another element to form two different compounds is the ratio of two small whole numbers

A

Law of multiple proportions

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3
Q

Composed of atoms held together in molecules by covalent bonds

A

Molecular compound

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4
Q

What are the building blocks of molecular compounds?

A

Molecules containing atoms of 2 Nonmetals

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5
Q

A bond between two atoms created by sharing one of more pairs of electrons

A

Covalent bond

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6
Q

Nonmetal oxides found in atmosphere

A

CO2, H2O, SO3, SO2, NO

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7
Q

A notation showing the number and type of atoms present in one molecule of a molecular compound

A

Molecular formula

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8
Q

A compound composed of positively and negatively charged ions held together by electrostatic attraction

A

Ionic compound

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9
Q

What two things form an ionic compound?

A

Metallic element and nonmetal

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10
Q

A positively charged particle created when an atom of molecule loses one or more electrons

A

Cation

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11
Q

A negatively charged particle created when an atom or molecule gains one of more electrons

A

Anion

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12
Q

A formula showing the smallest whole number ratio of elements in a compound

A

Empirical formula

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13
Q

The smallest electrically neutral unit of an ionic compound

A

Formula unit

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14
Q

Group 1 of periodic table

A

Lose 1 electron and form 1+ ions

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15
Q

Group 2 of periodic table

A

Lose 2 electrons and form 2+ ions

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16
Q

Group 13 of periodic table

A

Lose 3 electrons and form 3+ ions

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17
Q

As metallic elements lose electrons in forming ionic compounds, their nonmetallic partners (blank) so overall charge = zero

A

Gain them

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18
Q

Group 17 of periodic table

A

1-

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19
Q

Group 16 of periodic table

A

2-

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20
Q

Group 15 of periodic table

A

3-

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21
Q

Steps for molecular formula of a binary molecular compound to form a compound name

A

1) start with name of first element in formula
2) change ending of name of second element to -ide
3) add prefixes to indicate # of atoms

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22
Q

Prefix for naming compounds and writing formulas: 1

A

mono

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23
Q

Prefix for naming compounds and writing formulas: 2

A

Di

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24
Q

Prefix for naming compounds and writing formulas: 3

A

Tri

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25
Q

Prefix for naming compounds and writing formulas: 4

A

Tetra

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26
Q

Prefix for naming compounds and writing formulas: 5

A

Penta

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27
Q

Prefix for naming compounds and writing formulas: 6

A

Hexa

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28
Q

Prefix for naming compounds and writing formulas: 7

A

Hepta

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29
Q

Prefix for naming compounds and writing formulas: 8

A

Octa

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30
Q

Prefix for naming compounds and writing formulas: 9

A

Nona

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31
Q

Prefix for naming compounds and writing formulas: 10

A

Deca

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32
Q

Prefix for naming compounds and writing formulas: 11

A

Undeca

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33
Q

Prefix for naming compounds and writing formulas: 12

A

Dodeca

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34
Q

A pure substance composed of two or more elements

A

Compound

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35
Q

Types of compounds

A

Ionic and molecular

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36
Q

Consist of ions

A

Ionic compounds

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37
Q

Consist of molecules

A

Molecular compounds

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38
Q

Smallest unit of a molecular compound that retains the characteristic of that compound

A

Molecule

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39
Q

Indicates the # of atoms of each type within a molecule

A

Molecular formula

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40
Q

Sticks in ball and stick model

A

Covalent bonds

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41
Q

What hold the balls together in a molecule

A

Covalent bonds

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42
Q

A molecular formula that shows structural information and/or groups of atoms

A

Condensed formula

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43
Q

Representation of how atoms are attached within a molecule

A

Structural formula

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44
Q

Charged groups of two or more atoms joined together by covalent bonds

A

Polyatomic ions

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45
Q

Polyatomic ions that contain oxygen in combination with one or more other elements

A

Oxoanions

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46
Q

Compounds that highlight particular chemical properties

A

Acids

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47
Q

What release hydrogen ions when they dissolve in water?

A

Acids

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48
Q

Steps to name binary acids

A

1) add prefix hydro to name of element and replace last syllable with ic + acid

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49
Q

Mass of one molecule of a molecular compound

A

Molecular mass

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50
Q

The mass of one formula unit of an ionic compound

A

Formula mass

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51
Q

Hold together atoms within a molecule

A

Intramolecular forces

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52
Q

Forces between neighboring molecules

A

Intermolecular forces

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53
Q

Used to provide profiles of structures rather than images of single molecules

A

Atomic force microscopy

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54
Q

How do we determine the mass (in grams per mole) of a molecule like ethanol or water?

A

Molecular weight

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55
Q

Sum of atomic weights of all atoms in a molecule

A

Molecular weight

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56
Q

What is another term for molecular weight?

A

Molar mass

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57
Q

Atoms or groups of atoms with a positive or negative charge

A

Ions

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58
Q

Form when atoms lose one or more electrons

A

Cations

59
Q

Form when an atom gains one or more electrons

A

Anions

60
Q

What are the general rules for predicting ion charges?

A
  • metals lose electrons to form cations

- Nonmetals gain electrons to form anions

61
Q

By losing or gaining electrons, atoms have the same # of electrons as the nearest group (blank) atom

A

8A atom

62
Q

1A ion charge

A

+1

63
Q

2A ion charge

A

+2

64
Q

3A ion charge

A

+3

65
Q

4A ion charge

A

-4

66
Q

5A ion charge

A

-3

67
Q

6A ion charge

A

-2

68
Q

7A ion charge

A

-1

69
Q

Transition metals charges

A

Widely variable

70
Q

An ion consisting of more than one atom

A

Polyatomic ions

71
Q

Steps for naming a binary ionic compound

A

1) start with name of cation
2) add name of anion (name of element with ending ide)
No prefixes
Electrically neutral

72
Q

Name SrCl2

A

Strontium chloride

73
Q

Name NaF

A

Sodium fluoride

74
Q

Name MgO

A

Magnesium oxide

75
Q

Name CaBr2

A

Calcium bromide

76
Q

Write the formulae for aluminum oxide

A

Al2O3

Charges switch when forming subscripts

77
Q

Techniques for the separation of mixtures

A

Chromatography

78
Q

Formulas of ionic compounds- ionic compounds should have (blank) net charge

A

No

Sum of + and - = 0

79
Q

Steps for naming ionic compounds

A

1) name the positive ion first (cation) followed by the negative ion (anion)

80
Q

What are the negative ions?

A 
H-
C4-
N3-
O2-
F-
P3-
S2-
Cl-
Se2-
Br-
Te2-
I-
81
Q

Fe2+

Iron (II) ion

A

Ferron

82
Q

Fe3+

Iron (III) ion

A

Ferric

83
Q

Name CaF2

A

Calcium fluoride

84
Q

Name Mg(NO3)2

A

Magnesium nitrate

85
Q

Name Fe3(PO4)2

A

Iron (II) phosphate

86
Q

KBr

A

Potassium bromide

87
Q

Li2CO3

A

Lithium carbonate

88
Q

Coulombs law in words

A

Cations and anions are attracted to each other by electrostatic forces

89
Q

As ion charge increases, the attractive force (blank)

A

Increases

90
Q

As the distance between the ions increases, the attractive force (blank)

A

Decreases

91
Q

Properties of ionic compounds

A
  • exist as 3D arrays of anions and cations
  • cations surrounded by anions and vice versa
  • tend to be transparent, hard, and brittle as crystalline solids
92
Q

Bonding =

A

Electron sharing

93
Q

Molecular compounds formed between

A

2 nonmetals

94
Q

Rules for naming molecular compounds

A

1) first element in formula is named first, using full element name
2) name the second element as if it were an anion (ide)
3) prefixed are used to denote the number of atoms present
4) prefix mono never used for first element

95
Q

Name NI3

A

Nitrogen triiodide

96
Q

SF6

A

Sulfur hexafluroride

97
Q

P4O10

A

Tetraphosphorus decoxide

98
Q

02F2

A

Dio y gen difluoride

99
Q

The composition of a compound expressed in terms of the percentage by mass of each element in the compound

A

Percent composition

100
Q

% composition equation

A

Mass of element / molar mass x 100

101
Q

Mass in grams of 1 mole of a compound

A

Molar mass

102
Q

How to find the mass percent of an element:

A

Mass of element / total mass of the compound

103
Q

Formula determined from percent composition

A

Empirical formula

104
Q

Steps to find the empirical formula from % composition

A

1) assume 100 g of substance, % values = mass values, add % to 100
2) convert mass to moles
3) compute mole ratio by reducing one of the mole values to 1
4) convert ratio into whole #s if necessary

105
Q

Represent the relative proportions of the ions in the formula unit of an ionic compound

A

Empirical formulas

106
Q

The key to translating empirical formulas into molecular formulas is to determine the (blank) and the key to determining this is knowing the (blank)

A

Value of n

Molecular mass

107
Q

Who came up with the mass spectrometer?

A

Francis Aston

108
Q

An instrument that separates and counts ions according to their mass

A

Mass spectrometer

109
Q

A graph of the data from a mass spectrometer, where m/z ratios of the deflected particles are plotted against the # of particles with a particular mass

A

Mass spectrum

110
Q

The peak of the highest mass in a mass spectrum; it has the same mass as the molecule from which it came

A

Molecular ion (M+)

111
Q

Simplest whole number ratio of elements in a compound

A

Empirical formula

112
Q

How do you determine the molecular formula?

A

Obtain the molar mass of the compound experimentally (mass spectrometer)

113
Q

What are the 3 steps to get a molecular formula?

A

1) get exp data
2) determine the mass of the empirical formula
3) find the ratio of the mass

114
Q

Ionic compounds having water molecules trapped in their lattice

A

Hydrated compounds

115
Q

Compounds without water (may be obtained by heating)

A

Anhydrous compounds

116
Q

The quantitive relation between reactants and products in a chemical reaction

A

Stoichiometry

117
Q

The sum of the masses of the reactants in a chemical reaction is equal to the sum of the masses of the products

A

Law of conservation of mass

118
Q

A class of organic compounds composed of only hydrogen and carbon

A

Hydrocarbons

119
Q

A heat-producing reaction between oxygen and another element or compound

A

Combustion reaction

120
Q

What are the only products when the combustion of a hydrocarbon is complete?

A

Carbon dioxide and water

121
Q

What are key reactions in the carbon cycle?

A

Photosynthesis and respiration

122
Q

What two things do we need to know to determine mass of any substance involved in any chemical reaction?

A

1) mass of another substance in reaction

2) stoichiometric relation between 2 substances

123
Q

Chemical equations indicate

A

The kind of reactants and produces

Relative amounts of reactants and products

124
Q

The relationship between the amount of chemical reactants and products

A

Stoichiometry

125
Q

The numbers in front of reactants and products

A

Stoichiometric coefficients

126
Q

S, g, l, aq represent

A

Physical states of reactants and products

127
Q

Matter can neither be created nor destroyed

A

Law of conservation of matter

128
Q

The burning of organic compounds (fuel) in oxygen with the evolution of heat, CO2, and H2O

A

Combustion reaction

129
Q

Steps to balance combustion reactions

A

1) write out correct formulas for reactants and products
2) balance C atoms
3) balance H atoms
4) balance O atoms
5) check work

130
Q

The study of the quantitative aspects of chemical reactions

A

Stoichiometry

131
Q

Stoichiometry problems should be attempted only when you have a (blank) chemical equation

A

Balanced

132
Q

Maximum quantity of product that can be produced in a reaction

A

Theoretical yield

133
Q

General plan for stoichiometry calculations

A

Mass reactant- moles reactant- stoichiometric factor- moles product- mass product

134
Q

Percent yield

A

(Actual yield / theoretical yield)x100

135
Q

A reactant that is consumed completely in a chemical reaction

A

Limiting reactant

136
Q

The maximum amount of product possible in a chemical reaction for given quantities of reactants

A

Theoretical yield

137
Q

The amount of product obtained from a chemical reaction, which is often less than the theoretical yield

A

Actual yield

138
Q

The ration, expressed as a %, of the actual yield of a chemical reaction to the theoretical yield

A

Percent yield

139
Q

The reagent in short supply (blank) the quantity of product that can be formed

A

Limits

140
Q

Limiting reagent =

A

Limiting reactant

141
Q

What are the two types of limiting reagent problems?

A

1) 1:1 ratio of reactants

2) non 1:1 ratios of reactants

142
Q

Limiting reagent dictates (blank)

A

Theoretical yield

143
Q

A laboratory procedure for determining the composition of a substance by burning it completely in oxygen to produce known compounds whose masses are used to determine the composition of the original material

A

Combustion analysis

144
Q

Combustion analysis yield the percentages by mass of all atoms in a sample except (blank)

A

Oxygen

Chemisty (10 decks)

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