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Chemistry Flashcards

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1
Q

the study of the composition, structure, and properties of matter

A

Chemistry

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2
Q

anything that occupies space and has mass

A

Matter

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3
Q

the amount of matter in an object (expressed in g, kg, tons, pounds)

A

Mass

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4
Q

the gravitational force on an object (expressed in Newton)

A

Weight

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5
Q

formula for weight

A

Weight = mass x gravity (W=mg); gravity (Earth) = 9.8 m/s^2

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6
Q

exact space occupied by an object; Impenetrability property: no two objects can occupy the same space at the same time

A

Volume

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7
Q

the amount of matter in a given volume of material (expressed in g/cm^3 or kg/m^3)

A

Density

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8
Q

formula for density

A

Density = mass/volume (D=m/V)

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9
Q

matter is composed of particles called atoms

A

Atomic Theory

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10
Q

the basic building blocks that makeup matter; smallest particle

A

Atom

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11
Q

Atom is from a Greek word ______ that means _____

A

atomos = indivisible

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12
Q

What are atoms made up of?

A

protons (+), electrons (-), neutrons (no charge)

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13
Q

What subatomic particles are on the inside of the nucleus?

A

protons and neutrons

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14
Q

What subatomic particle is residing around the nucleus?

A

electrons

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15
Q

atomic number: number of ______

A

protons

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16
Q

atomic model that stated the atom is hard and indestructible

A

Billiard Ball Model

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17
Q

Who is the scientist behind Billiard Ball Model?

A

John Dalton

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18
Q

this atomic model shows electrons embedded in a positively-charged sphere

A

Plum Pudding Model

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19
Q

Who is the scientist behind Plum Pudding Model?

A

JJ Thompson

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20
Q

In this atomic model, the mass and all of the positive charge of an atom is concentrated in the nucleus

A

Nuclear Model

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21
Q

Who is the scientist behind the Nuclear model?

A

Ernest Rutherford

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22
Q

In this atomic model, electrons travel around the nucleus in a circular orbit; their energy is proportional to their distance form the nucleus

A

Planetary Model

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23
Q

Who is the scientist behind the Planetary model?

A

Niels Bohr

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24
Q

In this atomic model, the electron is a wave; found in orbitals

A

Quantum Model

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25
Q

Who is the scientist behind the Quantum model?

A

several scientists but Erwin Schrodinger is the most relevant

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26
Q

form of matter with a constant composition

A

Pure substances

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27
Q

How can elements and compounds be pure substances?

A

because their composition is always fixed, and their constituents can only be separated using chemical or electrochemical reactions

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28
Q

simplest form of matter, cannot be broken down into smaller components

A

Elements

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29
Q

How many elements were currently known to man?

A

118 elements

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30
Q

Who created the Periodic Table of Elements, and when did he create it?

A

Dmitri Mendeleev in 1869

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31
Q

What is the most common and lightest element in the universe?

A

Hydrogen

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32
Q

What is the second most abundant element, although it is very rare on Earth?

A

Helium

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33
Q

What is the most common element on Earth by its mass?

A

Oxygen

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34
Q

What is the first man-made element?

A

Technetium

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35
Q

charged atom

A

Ion

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36
Q

negatively-charged; gain electrons; electrons>protons

A

Anion

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37
Q

positively-charged; loss of electrons; electrons<protons

A

Cation

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38
Q

energy required to remove an electron from an atom

A

Ionization energy

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39
Q

energy released when an electron is added to an atom

A

Electron Affinity

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40
Q

ability to attract electrons

A

Electronegativity

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41
Q

lustrous, malleable (can be pounded into thin sheets), good conductor of heat and electricity

A

Metals

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42
Q

What are some of the metal elements?

A

aluminum, iron, gold, cooper, mercury, lead

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43
Q

poor conductor of heat and electricity, brittle

A

Non-metals

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44
Q

What are some of the non-metal elements

A

carbon, oxygen, hydrogen, phosphorus

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45
Q

have some characteristics of either metals or non-metals

A

Metalloid

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46
Q

What are some examples of metalloid elements?

A

silicone, boron, arsenic

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47
Q

highly reactive metals; have one excess electron which they tend to lose, thus they usually have a charge of +1; usually from compounds with halogens

A

Alkali metals

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48
Q

highly reactive non-metals; lack one electron on their outer shell which they try to acquire from other atoms, thus they usually have a charge of -1; usually forms compounds with alkali metals

A

Halogens

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49
Q

inert gases; unreactive, very stable elements owing to their full outer shell of eight electrons

A

Noble gases

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50
Q

elements to the right of metalloids (except H)

A

Non-metals

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51
Q

elements to the left of metalloids (except H

A

Metals

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52
Q

atoms of the same element that differ in the number of neutrons

A

Isotopes

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53
Q

describes how electrons are distributed in its atomic orbitals

A

Electron Configuration

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54
Q

the number of “excess” electrons in an atom

A

Valence electrons

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55
Q

every element has the same electronic configuration as the element before it in the periodic table, plus one extra

A

Aufbau principle

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56
Q

electrons tend to stay unpaired in orbitals with equal energies

A

Hund’s rule

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57
Q

members of a family of an element that all have the same number of protons but different numbers of neutrons

A

Isotopes

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58
Q

two or more elements with atoms bonded together

A

Compounds

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59
Q

How can compounds be separated?

A

Chemical Methods

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60
Q

carbon-containing compounds (e.g. sugar, acetone, methane)

A

Organic compounds

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61
Q

compounds with no carbons (e.g. salt, lye, water)

A

Inorganic compounds

62
Q

a characteristic sour taste

A

Acids

63
Q

Acids litmus test

A

blue to red

64
Q

acids pH level

A

less than 7; the lower the pH, the more acidic

65
Q

What do acids yield?

A

hydrogen ions

66
Q

has a litmus test of red to blue

A

bases

67
Q

pH level of bases

A

between 7-14

68
Q

What do bases yield?

A

hydroxide ions

69
Q

no litmus test changes

A

neutrals

70
Q

sodium and chlorine compound

A

table salt (NaCl)

71
Q

one carbon atom and two oxygen atoms

A

Carbon dioxide (CO2)

72
Q

6 carbon atoms, 12 hydrogen atoms, 6 oxygen atoms

A

Sugar/glucose (C6H12O6)

73
Q

formed by a cation and an anion wherein there is a transfer of electrons so that each atom has the same number of electrons as the nearest noble gas (so it is more stable)

A

Ionic Compound

74
Q

the compound formed by atoms that share electrons so that each atom has the same number of electrons as the nearest noble gas

A

Covalent Compound

75
Q

two types of chemical bonding

A

Intramolecular and Intermolecular

76
Q

attraction between atoms in a molecule

A

Intramolecular

77
Q

2 types of intramolecular

A

Covalent bond and Ionic bond

78
Q

attraction between molecules

A

Intermolecular

79
Q

3 types of intermolecular

A

London dispersion forces, dipole-dipole forces, hydrogen bond

80
Q

sharing of electrons between two non-metals

A

Covalent bond

81
Q

transfer of electrons; between metals and non-metals/cations and anions

A

Ionic bond

82
Q

between two temporarily polar molecules

A

London dispersion forces

83
Q

or polar covalent molecules

A

Dipole-dipole forces

84
Q

between the H atom of one molecule and an N,F, or O atom of another molecule

A

Hydrogen bond

85
Q

VSEPR

A

Valence Shell Electron Pair Repulsion

86
Q

shapes of molecules depend on the fact that electron pairs tend to move as far apart from one another as possible

A

VSEPR

87
Q

having a partial positive and partial negative ends, or poles

A

Polar molecule

88
Q

when a liquid is soluble in another liquid; the liquid present larger quantity is solvent

A

Miscible

89
Q

combination of two pure substances

A

Mixtures

90
Q

appears as one uniform material with uniform characteristics

A

Homogeneous mixture

91
Q

universal solvent

A

water

92
Q

the ______ the solvent, the more solute would be dissolves

A

warmer

93
Q

two parts of a solution

A

solvent and solute

94
Q

the part of a solution that dissolves

A

solvent

95
Q

the part of a solution that is dissolved

A

solute

96
Q

types of solutions

A

unsaturated, saturated, supersaturated

97
Q

type of solution that can still dissolve more solute

A

unsaturated

98
Q

type of solution that already contains the maximum amount of solute

A

saturated

99
Q

type of solution that is used to pressure or heat to dissolve more than the usual amount of solute

A

supersaturated

100
Q

does not have uniform particles, therefore the particles could be identified individually

A

Heterogeneous mixture

101
Q

its particles are larger than those in a solution, so the particles often settle in the bottom of the solvent

A

suspension

102
Q

in between being a homogeneous and heterogeneous mixture

A

Colloids

103
Q

the scattering of light exhibited by a colloid mixture

A

The Tyndall Effect

104
Q

Ideal Gas Law formula

A

pV = nRT

105
Q

decreasing the volume increases collisions and increases pressure

A

Boyle’s Law

106
Q

Boyle’s law formula

A

p1V1 = p2V2

107
Q

increasing the temperature increases volume

A

Charles’ Law

108
Q

Charles’ law formula

A

V1/T1 = V2/T2

109
Q

increasing the temperature increases pressure

A

Gay-Lussac’s Law

110
Q

Gay-Lussac’s law formula

A

p1/T1 = p2/T2

111
Q

Combined Gas law formula

A

p1V1/T1 = p2V2/T2

112
Q

Avogadro’s law formula

A

V1/n1 = V2/n2

113
Q

the number of units in one mole of any substance

A

Avogadro’s number: 6.02214076 x 10^23

114
Q

measure the dimensions then compute using formulas

A

Regular solids

115
Q

water displacement

A

Irregular solids

116
Q

use a graduated cylinder

A

Liquids

117
Q

no definite volume, pressure is usually measured instead

A

Gases

118
Q

particles in gas are infinitely small and are in constant random motion; gases do not experience intermolecular forces

A

The Kinetic Molecular Theory of Gases

119
Q

according to the Kinetic Molecular Theory of Gases, gas molecules undergo to this as they bounce perfectly to one another

A

perfectly elastic collisions

120
Q

the kinetic energies of gas molecules are directly proportional to their what?

A

temperatures (the hotter, the faster the molecules move)

121
Q

Law of Thermodynamics where energy can neither be created nor destroyed; it can only change forms

A

1st Law (Conservation of Energy)

122
Q

Law of Thermodynamics where entropy of an isolated system always increases; entropy, or S, is the degree of disorder

A

2nd Law

123
Q

Law of Thermodynamics where entropy at -273.15K (absolute zero temperature) is zero; there can be no temperature lower than absolute zero

A

3rd Law

124
Q

enthalpy is the heat transferred between system and surroundings at constant pressure

A

Hess’ Law

125
Q

the amount of energy needed to raise the temperature of a substance by one degree; in J/kg-C; decreases as mass and temperature to be attained increases

A

Specific heat

126
Q

hotness or coldness

A

temperature

127
Q

total kinetic energy of molecules

A

heat

128
Q

temperature where liquid turns into gas; requires the addition of heat

A

Boiling point

129
Q

boiling point of water

A

100 degrees Celsius

130
Q

the temperature where solid becomes liquid; this change from solid to liquid requires heat

A

Melting Point

131
Q

melting point of water

A

0 degrees Celsius

132
Q

two or more compounds combine to form one compound

A

Combination reaction

133
Q

the opposite of a combination reaction - a complex molecule breaks down to make simpler ones

A

Decomposition reaction

134
Q

two solutions of soluble salts are mixed resulting in an insoluble solid forming

A

Precipitation reaction

135
Q

A + B -> AB

A

combination reaction

136
Q

AB -> A + B

A

decomposition reaction

137
Q

A + Soluble salt B -> Precipitate + Soluble salt C

A

precipitation reaction

138
Q

an acid and a base react with each other; generally, the product of this reaction is salt and water

A

Neutralization reaction

139
Q

Acid + Base -> Salt + Water

A

neutralization reaction

140
Q

oxygen combines with a compound to form carbon dioxide and water; these reactions are exothermic meaning they give off heat

A

combustion reaction

141
Q

A + O2 -> H2O + CO2

A

combustion reaction

142
Q

one element takes place with another element in the compound

A

displacement reaction

143
Q

A + BC -> AC + B

A

displacement reaction

144
Q

factors that increase rates of reactions

A

higher temperatures, higher concentration of reactants, larger surface area of reactants, addition of catalyst (substance that increases the rate of reaction without itself being consumed)

145
Q

factors that affect solubility

A

temperature, surface area of solutes, pressure

146
Q

mole fraction

A

moles solute/moles solution

147
Q

mass percentage

A

mass solute/mass solute x solvent x 100% (not sure)

148
Q

mass-volume percentage

A

(mass of solute/volume of solvent) x 100%

149
Q

volume-volume percentage

A

volume of solute/volume of solvent x 100%

150
Q

Molarity (M)

A

moles solute/volume of solution (L)

151
Q

Molality (m)

A

moles solute/mass of solvent (kg)

SCIENCE (3 decks)

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