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Chemistry 121 > Midterm 1 > Flashcards

Midterm 1 Flashcards

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1
Q

matter

A

anything that exhibits the property of intertia (has mass)

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2
Q

chemistry

A

the study and investigation of the structure and properties of matter

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3
Q

as you go down the periodic table…

A

elements express more metallic behavior

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4
Q

left side of periodic table

A

metals

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5
Q

right side of periodic table

A

nonmetals

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6
Q

scientific method steps

A

1) observation 2) formulate hypothesis 3) experimentation 4) theorize

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7
Q

hypothesis

A

a possible explanation for an observation; untested

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8
Q

theory

A

a set of tested hypotheses that gives an overall explanation of some natural phenomenon (the WHY), dynamic

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9
Q

law

A

summarizes of observations/what happens, do NOT change very often if ever

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10
Q

law of conservation of mass

A

in a chemical reaction, matter is neither created nor destroyed

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11
Q

SI base units

A

kg, meter, second, Kelvin, ampere, mole, candela

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12
Q

1 lb

A

453.59g

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13
Q

1 in

A

2.54cm

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14
Q

1 US gallon

A

3.785L

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15
Q

weight

A

measure of force, dependent on the body acting upon the object, changes by location in universe

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16
Q

mass

A

property of matter, remains the same throughout the universe

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17
Q

uncertain digit

A

rightmost digit in a recorded number, uncertainty is +/- 1 unless otherwise noted

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18
Q

accuracy

A

refers to the agreement of a given value to the TRUE value

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19
Q

precision

A

refers to the degree of agreement among several measurements of the SAME quantity

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20
Q

leading zeros

A

zeros to the left of the leftmost nonzero digit; NOT sig figs

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21
Q

captive zeros

A

zeros between nonzero digits; ALWAYS sig figs

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22
Q

trailing zeros

A

zeros right of the rightmost nonzero digit, significant and count ONLY if the number contains a decimal point

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23
Q

multiplication/division rounding rule

A

answer contains the same total number of sig figs as the number with the least number of sig figs for the numbers involved in the computation

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24
Q

addition/subtraction rounding rule

A

answer contains the same number of decimal places as the number that had the least number of decimal places for number involved in the computation

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25
Q

when to change rounding rules

A

when you change operation type

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26
Q

Kelvin to Celsius conversion

A

Tk=Tc + 273.15

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27
Q

Fahrenheit to Celsius conversion

A

Tc = (5/9)(Tf-32)

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28
Q

density equation

A

d = m/v

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29
Q

solid

A

rigid, fixed volume and shape

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30
Q

liquid

A

fixed volume but no fixed shape

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31
Q

gas

A

no fixed volume or shape

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32
Q

homogeneous mixture (solution)

A

visibly indistinguishable parts

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33
Q

heterogeneous mixture

A

visibly distinguishable parts

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34
Q

pure substance

A

substance with a constant composition of one component

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35
Q

compound

A

substance with constant composition that can be broken down to elements by chemical processes

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36
Q

element

A

substance that cannot be decomposed into simpler substances by chemical or physical means

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37
Q

law of definite proportion

A

a given compound always contains exactly the same proportion of elements by mass (Joseph Proust)

38
Q

law of multiple proportions

A

when two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers (John Dalton)

39
Q

Dalton’s Atomic Theory

A

1) each element is made of atoms 2) the atoms of a given element are identical; the atoms different elements are different in fundamental ways 3) chemical compounds are formed when atoms of different element combine with each other 4) chemical reactions involve the reorganization of the atoms, atoms themselves don’t change

40
Q

Joseph Gay-Lussac

A

observed at the same temperature and pressure 2 volumes of H gas reacted with one volume O gas

41
Q

Amedeo Avogadro

A

said at the same temperature and pressure that equal volumes of different gases contain the same number of particles

42
Q

J.J. Thomson

A

cathode-ray tube experiment; discovered electrons/charge to mass ratio of electron (-1.76 * 10^8 C/g), plum pudding model of atom (electrons in positive sphere of charge)

43
Q

Robert Millikan

A

oil drop experiment; determined magnitude of electron charge, used it and charge to mass ratio to find mass of an electron (9.11*10^-31 kg)

44
Q

radioactivity

A

found by Henri Becquerel and Marie Curie; in order of least to most energy: alpha particles (He nucleus), Beta particles (high speed electrons), gamma rays (high energy light)

45
Q

Ernest Rutherford

A

tested plum pudding model (proved it wrong), gold foil experiment, saw some alpha particles bounced back at the source/high angle deflection, made nuclear model of atom (dense center of positive charge with electrons moving around nucleus)

46
Q

protons

A

positive charge, equal but opposite in magnitude to electron charge

47
Q

neutrons

A

have NO charge, about the same mass as a proton

48
Q

atoms

A

no net charge, number of protons and electrons EQUAL

49
Q

isotopes

A

atoms or ions with the same number of protons but DIFFERENT numbers of neutrons

50
Q

atomic number (Z)

A

number of protons

51
Q

Mass number (A)

A

sum of protons and neutrons in nucleus

52
Q

ion

A

atom or group of atoms with a net positive or negative charge

53
Q

cation

A

positively charged ion

54
Q

anion

A

negatively charged ion

55
Q

ionic solid (salt)

A

solid made of oppositely charged ions, can be simple (K+) or polyatomic (NO3-)

56
Q

metals

A

tend to be conductive, malleable, lustrous and ductile elements, tend to LOSE electrons

57
Q

non-metals

A

tend to be non-conductors, brittle, not lustrous, tend to GAIN electrons

58
Q

groups/families

A

elements in the same vertical column

59
Q

alkali metals

A

form 1+ cations

60
Q

alkaline earth metals

A

form 2+ cations

61
Q

halogens

A

form 1- anions

62
Q

noble gases

A

usually don’t like to gain or lose electrons, usually monoatomic

63
Q

periods

A

elements in the same horizontal rows on the periodic table

64
Q

mass spectrometer

A

used to determine atomic masses

65
Q

Carbon-12

A

used as standard for all atomic masses, other masses are relative to it

66
Q

mole

A

number of carbon atoms in exactly 12 grams of pure carbon-12

67
Q

Avogadro’s number

A

6.022 * 10^23 (atoms or molecules per mole)

68
Q

chemical bonds

A

forces that hold atoms together in compounds

69
Q

covalent bonds

A

sharing electrons to bond together; also called a molecule

70
Q

empirical formula

A

smallest whole number ratio of elements in a compound (ex. CH3)

71
Q

molecular formula

A

number and type of elements needed to represent one complete molecule of a compound (ex. C2H6)

72
Q

structural formula

A

individual bonds between atoms are shown (as a line), each line also represent the 2 electrons that make up the bond

73
Q

ball and stick model

A

shows atoms and their relative orientation to one another in the molecule

74
Q

space filling model

A

shows the relative size of atoms and their relative orientation in a molcule

75
Q

ionic bonds

A

forces of attraction between oppositely charged ions (cation + anion), usually stronger than covalent bond

76
Q

binary compound naming rules

A

1) cation is first, followed by anion 2) monoatomic cation takes its name from the name of the element (ex. sodium chloride)

77
Q

binary compound type 2

A

some metals have different positive charges, use roman numeral in name to indicate charge (ex. Iron (II) chloride and iron (III) chloride), IF MULTIPLE IONIC COMPOUNDS CAN FORM

78
Q

-ic

A

cation with higher charge (ex. Fe 3+ is ferric ion)

79
Q

-ous

A

cation with lower charge (ex. Fe 2+ is ferrous ion)

80
Q

transition metal charges

A

Ag+, Zn2+, Sc 3+, Al 3+,

81
Q

oxyanions

A

anions that contain oxygen

82
Q

binary covalent compounds

A

molecules formed by 2 atoms sharing valence electrons (usually 2 nonmetals), do NOT contain ions

83
Q

binary covalent compounds naming rule

A

1) 1st element is named first using full element name 2) second element named as if it were an anion 3) prefixes used to denote the numbers of atoms present; mono- NEVER used for naming the first element

84
Q

vowel drop rule

A

often the last letter of the prefix is dropped when it is followed by a vowel

85
Q

acid naming rule

A

1) if the anion does NOT have oxygen, it has the prefix hydro- and the suffix -ic 2) if there IS oxygen, the acidic name is formed from the root of the anion name with the suffix -ic or -ous 2a) if the anion ends in -ate, add -ic (ex. sulfate to sulfuric acid) 2b) if the anion has an -ite ending the -ite is replaced by -ous (ex. sulfite to sulfurous acid)

86
Q

hydrated ionic compounds (hydrates)

A

ionic compounds with a specific number of water molecules associated with the formula (ex. CuSO4 * 5 H2O is sulfate pentahydrate)

87
Q

molar mass (molecular weight)

A

the mass per mole of any material

88
Q

percent composition of compounds

A

two ways to describe are 1) in terms of the numbers of its constituent atoms and 2) in terms of the percentages (by mass) of its elements

89
Q

mass percentage method

A

compare the mass of the element in the compound to the total mass of the compound (ex. divide H2 by H2O to get 11.12% H in H2O)

90
Q

combustion analysis

A

completely incinerate a sample to determine the mass of all elements present

91
Q

reactants

A

on left side of arrow in chemical equation

92
Q

products

A

on right hand side of arrow in chemical reaction

Chemistry 121 (6 decks)

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