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Chemistry (Poohriffic!) > Chem Term Review > Flashcards

Chem Term Review Flashcards

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1
Q

the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons

A

metallic bonding

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2
Q

metals are composed of atom cores surround by free moving valence electrons. The electrons can more from one metal atom to another

A

electron sea model

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3
Q

created by slightly positive and negative charges (opposite charges) that are separated by a short distance.

A

dipole

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4
Q

the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule (i.e., H2O)

A

hydrogen bonding

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5
Q

the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles called this.

A

London dispersion forces

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6
Q

electrons that move freely about the electron sea (they do not have a “home” atom)

A

delocalized electrons

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7
Q

states that repulsion between the sets of valence-level electrons surrounding an atom cause these sets to be oriented as far apart as possible (it leads to molecular geometrical shapes)

A

VSEPR Theory

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8
Q

orbitals of equal energy produced by the combination of two or more orbitals on the same atom (carbon bonding)

A

hybrid orbitals

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9
Q

a pair of electrons of an atom that DO NOT bond

A

lone pair electrons

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10
Q

a covalent bond in which the bonded atoms have an unequal attraction for shared electrons (ex. HCl)

A

polar-covalent bond

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11
Q

chemical bond that results from the electrical attraction between cations and anions (the giving up of electrons)

A

ionic bond

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12
Q

a covalent bond in which the bonding of electrons are shared equally by the bonded atoms, resulting in a balanced distribution of an electrical charge (ex. H2)

A

nonpolar-covalent bond

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13
Q

a covalent bond in which one pair of electrons is shared between two atoms

A

single bond

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14
Q

a covalent bond in which two pairs of electrons is shared between two atoms

A

double bond

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15
Q

a covalent bond in which three pairs of electrons is shared between two atoms

A

triple bond

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16
Q

the ability of a substance to be hammered or beaten into thin sheats

A

malleability

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17
Q

forces between molecules

A

intermolecular forces

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18
Q

the ability of a substance to be drawn, pulled, or extruded through a small opening to produce

A

ductility

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19
Q

the simplest collection of atoms from an ionic compound’s formula can be established

A

formula unit

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20
Q

the 3-dimensional arrangement of + and - ions (like NaCl) in a complex shape

A

crystal lattice

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21
Q

Bond angle and name for NH3

A

107.5 trigonal pyramidal

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22
Q

Bond angle and name for H2O

A

104.5 bent or angular

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23
Q

Bond angle and name for CH4

A

109.5 tetrahedral (electrons farthest away from e/o here)

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24
Q

linear angle - give degrees

A

180

25
Q

Trigonal planar - give degrees

A

120

26
Q

an atom or molecule that has gain or lost one or more electrons and has a negative and positive charge

A

ion

27
Q

compound composed of ions bound together by electrostatic attraction (#anions = #of cations)

A

ionic compound

28
Q

a chemical compound whose simplest units are molecules

A

molecular compound

29
Q

a positive ion

A

cation

30
Q

a negative ion

A

anion

31
Q

an ion formed from a single atom

A

monatomic ion

32
Q

ion formed from multiple atoms

A

polyatomic ion

33
Q

the simplest collection of atoms from which an ionic compound’s formula can be established

A

formula unit

34
Q

the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula unit, or ion

A

formula mass

35
Q

a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound (ex H2O)

A

molecular formula

36
Q

the mass of one mole of a pure substance

A

molar mass

37
Q

the symbols for the elements combined in a compound with subscripts showing the smallest whole-number mole ratio of the different atoms in the compound

A

empirical formula

38
Q

a substance that reacts in a chemical change

A

reactant

39
Q

a substance that is formed by a chemical change

A

product

40
Q

Where is the subscript and coefficient?

A
41
Q

an equation that has the same amount of atoms on both sides

A

balanced equation

42
Q

the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12

A

mole

43
Q

the mass of one mole of a pure substance

A

molar mass

44
Q

a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction

A

mole ratio

45
Q

the reactant that limits the amounts of the other reactants that can combine—and the amount of product that can form—in a chemical reaction

A

limiting reactant

46
Q

the substance that is not used up completely in a reaction

A

excess reactant

47
Q

the maximum amount of product that can be produced from a given amount of reactant

A

theoretical yield

48
Q

the measured amount of a product obtained from a reaction

A

actual yield

49
Q

the ratio of the actual yield to the theoretical yield, multiplied by 100

A

percent yield

50
Q

force per unit area of a surface

A

pressure

51
Q

exactly equivalent to 760 mm Hg

A

atmosphere (pressure)

52
Q

the pressure exerted by a force of one newton acting on an area of one square meter

A

pascal

53
Q

the common unit of pressure measured from a mercury barometer

A

mm Hg

54
Q

a pressure of 1 mm Hg in honor of Torricelli’s barometer

A

torr

55
Q

the temperature -273.15C. is called this and is given a value of zero in the Kelvin scale

A

absolute zero

56
Q

the mathematical relationship among pressure, volume, temperature, and # of moles of a gas (PV = nRT)

A

ideal gas

57
Q

a collision where there is no net loss of total kinetic energy

A

elastic collision

58
Q

the conditions of exactly 1 atm pressure and 0C (273K)

A

standard temperature pressure (STP)

Chemistry (Poohriffic!) (15 decks)

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