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Chemistry > Vocab Final Exam > Flashcards

Vocab Final Exam Flashcards

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1
Q

Chemical bond

A

Mutual electrical attraction between nuclei and valence electrons of different atoms that binds the atoms together

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2
Q

Ionic bonding

A

Results from the electrical attraction between large numbers of cations and anions. atoms donate or accept electrons from each other

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3
Q

Covalent bonding

A

Results from sharing of electron pairs between 2 atoms. The electrons shared belong to both atoms

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4
Q

Polar covalent

A

When electrons are shared unevenly

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5
Q

Nonpolar covalent

A

When electrons are shared evenly

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6
Q

Ionic v. Covalent

A

Ionic: >1.7
Polar covalent: 0.3-1.7
Nonpolar covalent: 0-0.3
LOOK AT DIFFERENCE IN ELECTRONEGATIVITIES

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7
Q

Heat of sublimation

A

Amount of heat required to turn solid, bonded metal atoms into gaseous individual atoms

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8
Q

Properties of Metals

A

🔸conductivity
🔹luster(shininess)
🔸malleability & ductility

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9
Q

Octet Rule

A

A compound tends to form so that each atom has an octet(8) of electrons in its highest energy level by gaining, losing, or sharing electrons

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10
Q

Lewis dot structures

A

Like dot diagrams but for entire molecules, atomic symbols represent nucleus and core electrons and dots or dashes represent valence electrons

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11
Q

Double bonds

A

Sharing of 2 pairs of electrons; stronger and shorter

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12
Q

Triple bonds

A

Sharing of 3 pairs of electrons; strongest and shortest

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13
Q

Resonance

A

Bonding between atoms that cannnot be represented in on Lewis structure, shows all possible structures with double-ended arrow in between to show that electrons are delocalized

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14
Q

Single bond

A

Sharing of one pair of electrons; weakest and longest

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15
Q

Covalent network bonding

A

A different type of bonding, lots of nonmetal covalently bonded together in a network in all directions
Ex. Diamond, graphite, silicon dioxide

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16
Q

VSPER Theory

A

Valence, Shell, Electron, Pair, Repulsion
Repulsion between oaurs of electrons around an atom cause them to be as far apart as possible; used to predict the geometry of molecules

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16
Q

Intermolecular forces

A

Forces of attraction between molecules, vary in strength depending on type of molecule. Polar molecules have stronger IMF’s than nonpolar molecules. Are usually weaker than intramolecular forces( bonds inside a molecule)

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17
Q

Dipoles

A

A polar molecule( with an imbalance in electrons) has a dipole moment. There is a + center and - center
Represented by an arrow pointing from + center to - center

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18
Q

Boiling Point

A

Is a good measure of intermolecular forces(between molecules). Forces must overcome the attractive forces between molecules to pull them away from each other and enter the gas phase. Greater the molecules’s attraction, the higher the BP

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19
Q

Dipole-dipole

A

When molecules with dipole moments line up to minimize repulsion and maximize attraction. Very weak compared to covalent and ionic bonds

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20
Q

Hydrogen Bonding

A

🔸happens between H, N, O, & F

🔹 very strong type of dipole-dipole attraction because bond is so polar and because atoms are so small

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21
Q

London dispersion forces

A

In every molecular compound, only important for nonpolar molecules and noble gas atoms
🔹 weak, short-lived
🔸caused by formation of temporary dipole moments

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22
Q

Ionic crystals

A

🔹sites in lattice contain ions
🔸hard, brittle
🔹high melting points
🔸 good insulators as solids

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23
Q

Subscripts

A

Give you the simplest ratio of atoms or the number of atoms in a molecule

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24
Q

Molar mass

A

Mass of one mole of pure substance, units: g/mol

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25
Q

Percent composition

A

Percentage of mass of each element in the compound

Mass of the element in sample/ total mass of sample • 100

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26
Q

Chemical equation

A

Represents identities and relative amounts of reactants and products in the chemical reaction

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27
Q

Evidence or chemical change

A

🔸heat or light
🔹gas bubbles
🔸precipitate
🔹color change

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28
Q

Word equations

A

Uses names instead of formulas

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29
Q

Coefficients

A

Specifies the relative number of moles and molecules involved in the reaction, used to balance the equation

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30
Q

Synthesis

A

Combining more than one reactant to make only one single product

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31
Q

Decomposition

A

Breaking apart one reactant to make more than one product

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32
Q

Single replacement

A

An element replaces a similar element in a compound

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33
Q

Double Replacement

A

Two similar elements switch places

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34
Q

Combustion

A

Combines with oxygen and releases energy in form of heat/ light
🔹H2O and usually CO2 as products

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35
Q

Limiting reactant

A

Reactant that limits the amount of product created; completely used up

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36
Q

Excess reactant

A

React not completely used up

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37
Q

Theoretical yield

A

Maximum amount of product possible

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38
Q

Actual yield

A

The measured amount formed in reaction

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39
Q

Percent yield equation

A

Actual yield/ theoretical yield • 100

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40
Q

Activity series

A

Used to predict whether single replacement reactions will occur, most actce is on top, an element can replace anything below it but not any above it

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41
Q

Kinetic-molecular theory

A

Based on the idea that particles of matter are always in motion, theory can be used to explain the properties of solids, liquids, & gases in terms of energy of particles and the forces that act between them

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42
Q

Ideal gas

A

Is a hypothetical gas that perfectly fits all the assumptions of KMT

43
Q

Elastic collision

A

Is one in where there is no net loss of total kinetic energy

44
Q

Fluids

A

Gases and liquids flow, therefore they are fluids

45
Q

Real gas

A

Is a gas that doesn’t behave completely according to the assumptions of KMT

46
Q

Surface tension

A

Force that pulls parts of a liquid’s surface together

47
Q

Capillary action

A

Attraction of surface of liquid to surface of a solid
Ex. Water & paper
Water & glass
Meniscus

48
Q

Enthalphy of vaporization

A

Energy required to vaporize 1 mole of a liquid at 1 atm; ENDOTHERMIC

49
Q

Freezing

A

Physical change of a liquid to solid by removal of heat

50
Q

Enthalphy of fusion

A

Heat required to be removed between liquid to a solid

51
Q

Vapor pressure

A

Liquid can be injected under inverted tube, part of the liquid evaporates to the top of Pvap can be determind by height of Hg(mercury)

52
Q

Volatile

A

Liquids with high vapor pressure, evaporate quickly, weak intermolecular forces

53
Q

Phase diagrams

A

Represents the phases as function of T and P

54
Q

Triple point

A

All 3 phases exist- all have same vapor pressure

55
Q

Critical point

A

Where if the temperature is increased, vapor can’t be liquefied no matter what pressure is applied. Only one fluid phase exsists that is called supercritical fluid

56
Q

Pressure equation

A

Force/ area

57
Q

Barometer

A

A device used to measure atmospheric pressure

58
Q

Dalton’s law

A

The total pressure of a gas mixture is the sum of the partial pressures of the component gases
Ptotal= Pvap + Pgas
COLLECTING GAS OVER WATER

59
Q

Boyle’s law

A

The V of fixed mass of gas varies inverseky with P at a constant T
P1V1= P2V2

60
Q

Charles’s Law

A

The V of fixed mass of gas at constant P varies directly with Kelvin T
V1/T1 = V2/T2

61
Q

Gay-Lussac’s Law

A

The P of fixed mass of gas at constant V varies directly with Kelvin T
P1/T1 = P2/T2

62
Q

Combined gas law

A

Relationship between P, V, and T of a fixed amount of gas

P1V1/T1 = P2V2/T2

63
Q

Avogadro’s law

A

The law states that equal volumes of gases at the same temperature and pressure contsin equal numbers of molecules
V=kn or V/n =k

64
Q

Standard molar volume

A

The volume occupied by one mole of gas at STP or 22.4L

65
Q

Ideal gas law

A

Mathematical relationship between pressure, volume, temperature, and number of moles of a gas
PV=nRT

66
Q

Ideal gas constant

A

Constant “R” = 0.0821 L•atm/ mol•K= 8.314 L•kPA/ mol•K= 62.4 L•mmHg/ mol•K

67
Q

Effusion

A

When gases escape through a tiny opening into a vaccum

68
Q

Diffusion

A

When gases mix automatically without being stirred

69
Q

Graham’s Law of Effusion

A

Rates of effusion of gases at a constant T and P are inverseky proportional to the square roots of their molar masses
Rate of effusionA/ Rate of effusionB = square root MB/MA

70
Q

Mole ratio

A

of moles of one substance to ratio of # of moles of another substance

71
Q

Sublimation

A

Solid to gas

72
Q

Condensation

A

Gas to liquid

73
Q

Vaporization

A

Liquid to gas

74
Q

Deposition

A

Gas to solid

75
Q

Boiling

A

Example of vaporization

76
Q

Freezing

A

Liquid to solid

77
Q

Melting

A

Solid to liquid

78
Q

Cations

A

Positive ions

79
Q

Anions

A

Negative ions

80
Q

Melting point

A

Solid and liquid phase exsist in equilibrum

81
Q

Freezing point

A

Water; 0C

82
Q

Standard Temperature and Pressure(STP)

A

Pressure: 1atm
Volume: 22.4L
Temperature: 273.15K

83
Q

Formula unit

A

Empirical formula of any ionic or covalent network solid compound used as an independent entity for stoichionetric calculations. Lowest whole number ratio of ions represented in an ionic compound

84
Q

Polyatomic ion

A

Is a charged chemical ion composed of 2 or more atoms covalently bonded

85
Q

Hybridization

A

Mixing atomic orbitals ino bee hybrid orbitals with different energies, shapes, etc. than the component atomic orbitals

86
Q

Binary compound

A

Is a chemical compound that contains exactly 2 different types of elements
Ex. Calcium chloride, sodium fluoride

87
Q

Oxyanion

A

Is an ion with the generic formua A xOz-y. Determined by the octet rule

88
Q

Monatomic ion

A

Is an ion consisting of a single atom

89
Q

Salt

A

NaCl; remaining solid is known as the anhydrous salt

90
Q

Oxidation number

A

Indicator of the degree of oxidation( loss of electrons) of an atom in a chemical compound

91
Q

Oxidation state

A

Hypothetical charge that an atom would have if all bonds to atoms of different elementd were 100% ionic, with no covalent component

92
Q

Precipitate

A

Solid formed when the reaction occurs in a liquid solution

93
Q

Reversible reaction

A

Chemical reaction where the reactants form products that, in turn, react together to give the reactants back

94
Q

Percent yield

A

Amount of product obtained in a chemical reaction

Actual yield/ theoretical yield •100

95
Q

Dissociation

A

General process in which molecules separate or split into smaller particles such as atoms, ions, or radicals

96
Q

Ionization

A

Any process by which electrically neutral atoms or molecules are converted to ions

97
Q

Net ionic equation

A

A chemical equation for a reaction which lists only those species participating in the reaction

98
Q

Spectator ion

A

Ion that exsists as a reactsnt and product in a chemical reaction

99
Q

Suspension

A

Heterogeneous mixture containing solid particles that are sufficiently large for sedimentation

100
Q

Molarity

A

Number of moles of solute per liter of solution

101
Q

Molality

A

Number of moles of soluter per kilogram of solvent

102
Q

Mole fraction

A

To be equal to the number of moles of a component divided by the total number of moles of a solution

103
Q

Mass percent

A

Shows the amount each element in a molecule contributed to the total molecular mass

104
Q

Atmospheric pressure

A

Pressure exerted by the weight of air in the atmosphere of Earth

105
Q

Manometer

A

Instrument for measuring the pressure acting on a column of fluid

106
Q

Amorphous solid

A

A solid which doesn’t exhibit crystalline structure.

Ex. Window glass, polystyrene

Chemistry (8 decks)

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