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General Chemistry > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

Atomic Theory

A
  • Everything is made of atoms
  • Atoms are the smallest whole unit of am element
  • Atoms combine with like and different atoms to form molecules
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2
Q

Chemical Reaction

A
  • Chemicals interact to form different substances with different properties
  • Reordering of atoms
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3
Q

Chemical Property

A
  • describes a chemical change that a substance undergoes

- 2 types: intensive and extensive

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4
Q

Elements

A
  • Substances that cannot be decomposed into simpler materials by chemical reactions
  • Atoms all contain the same number of protons
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5
Q

Compound

A
  • Substance formed from two or more different elements in which the elements are always combined in the same fixed proportions by mass
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6
Q

Pure Substances

A
  • Element or compound
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7
Q

Mixture

A
  • Substance with variable composition

- Homogenous or heterogenous

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8
Q

Homogenous

A
  • Same properties throughout sample

- Solution

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9
Q

Heterogenous

A
  • Two or more phases with different properties

- i.e. oil and vinegar

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10
Q

Solution

A

Homogenous mixture

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11
Q

Mixture vs. Compound

A

No chemical change in a mixture. Chemical change in a compound.

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12
Q

Law of Conservation of Mass

A

Mass is conserved in chemical reactions

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13
Q

Law of Definite Proportions

A

In a given chemical compound, elements always combine in the same proportion by mass

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14
Q

Dalton’s Atomic Theory (know gist, do not need to memorize)

A
  1. Matter is made of atoms
  2. Atoms are indestructible and do not break apart
  3. In pure element samples, atoms identical in mass and properties
  4. Atoms of different elements differ in mass/ properties
  5. When atoms of different elements combine to form compounds, new and more complex particles form. However, in a given compound the constituent atoms are always present in a fixed numerical ratio.
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15
Q

Law of Multiple Proportions

A

Small whole numbers in ratios of elements in compounds

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16
Q

Atomic Mass

A
  • mass of a single atom
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17
Q

Atomic Weight

A
  • Listed on the P.T.

- Weighted average of masses of naturally occurring isotopes

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18
Q

Subatomic Particles

A

The stuff that makes atoms…. protons, electrons, neutrons

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19
Q

Atomic Number

A
  • The number of protons in an atom

- denoted by ‘Z’

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20
Q

Mass Number

A 
#p+#n 
denoted by 'A'
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21
Q

Mass Number

A 
#p+#n 
denoted by 'A'
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22
Q

Periods

A
  • Rows of periodic table
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23
Q

Groups

A
  • Columns of periodic table

- Numbered or roman-numeral-ed

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24
Q

Alkali Metals

A
  • Group IA (1)

+1

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25
Q

Alkali(ne) Earth Metals

A
  • Group IIA (2)

+2

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26
Q

Halogens

A
  • Group VIIA (17)

- 1

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27
Q

Noble Gases

A
  • Group VIIIA (18)

- do not form ions

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28
Q

Metalloid

A

Elements with properties that lie between those of metals and nonmetals. Tend to be semiconductors.

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29
Q

Metal

A
  • Good conductor of electricity
  • Shiny surface
  • Malleable
  • Ductile
  • Solid at room temp (except Mercury)
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30
Q

Nonmetal

A
  • Does not conduct electricity
  • Not malleable
  • Not ductile
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31
Q

Chemical Formulas

A
  • Chemical symbols used to represent atoms of elements present
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32
Q

Free Element

A
  • Element not combined with another - not in a compound

- All free nonmetal elements EXCEPT NGs exist as diatomic

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33
Q

Diatomic Molecules

A

Composed of 2 atoms each

H2,N2,O2,F2,Cl2,Br2,I2

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34
Q

Hydrates

A
  • Compounds whose crystals contain water molecules in fixed ratios
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35
Q

Dehydration

A

Removal of water

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36
Q

Chemical Equations

A
  • Describes what happens when a chemical reaction occurs

- MUST BE BALANCED

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37
Q

Energy

A
  • Something an object has if the object is able to do work
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38
Q

Kinetic Energy

A
  • The energy an object has while moving
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39
Q

Kinetic Energy Equation

A

KE = 1/2mv^2

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40
Q

Potential Energy

A
  • The energy an object has that can be changed to KE
  • Stored energy
  • PE of chemicals = chemical energy
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41
Q

Law of Conservation of Energy

A

Energy cannot be created or destroyed. It can only be transformed from one form to another

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42
Q

Temperature

A
  • Proportional to the average KE
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43
Q

Heat

A
  • Thermal energy
44
Q

Molecule

A
  • Electrically neutral particle consisting of two or more atoms
  • Held together by chemical bonds which are electrical in nature
45
Q

Molecular Formula

A
  • Denotes the number of each type of atom in a molecule
46
Q

Hydrides

A
  • Compounds that form with hydrogen
47
Q

Hydrocarbons

A
  • Compounds of H and C

- Usually follow rule of C(n)H(2n+n)

48
Q

Alkane

A
  • First six members of hydrocarbon series
49
Q

Inorganic Compounds

A

Do not derive from hydrocarbons

50
Q

Binary Compounds

A
  • Compounds composed of 2 different elements
51
Q

Ion

A

charged particle

52
Q

Ionic Compound

A
  • Formation involves electron transfers
  • Formed when metals react with nonmetals
  • Neutral charge
  • Do not call them molecules
  • In lattice form
53
Q

Formula Unit

A
  • A particle that has the composition given by chemical formula…. ie. NaCl
54
Q

Cation

A

Positive ion

55
Q

Anion

A

Negative ion

56
Q

Writing Ionic Compounds

A
  1. Positive ion first in formula
  2. Subscripts produce neutral formula unit
  3. Lowest whole # ratio
  4. Ion charges not included in finished formula
57
Q

Post-Transition Metals

A

Metals on the periodic table following a row of transition metals

58
Q

Polyatomic Ions

A
  • Ions composed of 2 or more atoms liked by the same kind of bonds that hold molecules together
59
Q

Proton

A
  • Subatomic particle
  • Positive charge
  • Massive (has mass)
  • Inside the nucleus
60
Q

Neutron

A
  • Subatomic particle
  • Neutral charge
  • Massive (has mass)
  • Inside nucleus
61
Q

Electron

A
  • Subatomic particle
  • ## Negative charge
62
Q

Electron

A
  • Subatomic particle
  • Negative charge
  • Negligible mass
  • Outside nucleus
63
Q

Inside vs. Outside Nucleus

A

Inside: where the mass is
Outside: where the volume is

64
Q

Transition Metals on the P.T.

A

Periods 4-7, groups 3-12 EXCEPT

P6,G3 and P7G3

65
Q

Actinide

A

Bottom period beginning in Ac

66
Q

Lanthanide

A

Second to bottom period beginning with La

67
Q

Non Metals on P.T.

A

H,C,N,O,P,S,Se

68
Q

Metalloid PT

A

B, Si, Ge, As, Sb, Te, Po

69
Q

States of Matter

A

Solid, liquid, gas
Solid most dense
Gas least dense

70
Q

Mono

A

1

71
Q

Di

A

2

72
Q

Tri

A

3

73
Q

Tetra

A

4

74
Q

Penta

A

5

75
Q

Hexa

A

6

76
Q

Hepta

A

7

77
Q

Octa

A

8

78
Q

Nona

A

9

79
Q

Deca

A

10

80
Q

Ionic Bonds

A
  • Form because of electrostatic attraction between oppositely charged ions
  • Metal and nonmetal
81
Q

Covalent Bonds

A
  • Sharing of electron in bond

- Between nonmetal and nonmetal

82
Q

Ammonia

A

NH3

not ammonium

83
Q

Hygroscopic

A

Absorbs water from the air

84
Q

Precipitate

A

Solids formed by a chemical reaction that drop out of solution

85
Q

Product

A

What is formed in a chemical reaction

86
Q

Reactant

A

What reacts in chemical reaction

87
Q

Aqueous

A
  • aq

- in solution

88
Q

Law of Constant Composition

A

Same compound = same composition.

89
Q

Mass percent

A

Mass element / compound

90
Q

Bonding

A

How we describe the way atoms are held together in atoms or compounds

91
Q

When bonds are formed, energy is….

A

RELEASED.

92
Q

When bonds are broken, energy is….

A

consumed.

93
Q

Lower energy state

A

more stable

94
Q

Binary Compound

A
  • contains only 2 elements

- only ionic

95
Q

Allotrope

A

Same element or compound in a different state

96
Q

In equations, metals tend to be

A

solid

97
Q

In equations, diatmoics tend to be

A

gas

98
Q

In equations, pure ionic compounds tend to be

A

solid

99
Q

In equations, pure ionic compounds with water are

A

aq

100
Q

In equations, hydrates are

A

solid

101
Q

Empirical Formula

A

Simplest, most reduced whole number ratio of atoms present in a chemical

102
Q

Mass Percent

A

(mass of element/mass of compound)*100

103
Q

Combustion

A

Reaction of substance and oxygen initiated with heat. Gives off more heat, CO2 and H2O.

104
Q

Avogadro’s Number

A

6.02x10^23

105
Q

Mole in words

A

Don’t worry about it. Just understand it.

106
Q

Molar Mass

A 
# grams in 1 mole of substance
- Sum of atomic masses of atoms in substance (in proper proportion)

General Chemistry (3 decks)

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