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Chemistry 121 > Midterm 1 > Flashcards

Midterm 1 Flashcards

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
when to change rounding rules
when you change operation type
26
Kelvin to Celsius conversion
Tk=Tc + 273.15
27
Fahrenheit to Celsius conversion
Tc = (5/9)(Tf-32)
28
density equation
d = m/v
29
solid
rigid, fixed volume and shape
30
liquid
fixed volume but no fixed shape
31
gas
no fixed volume or shape
32
homogeneous mixture (solution)
visibly indistinguishable parts
33
heterogeneous mixture
visibly distinguishable parts
34
pure substance
substance with a constant composition of one component
35
compound
substance with constant composition that can be broken down to elements by chemical processes
36
element
substance that cannot be decomposed into simpler substances by chemical or physical means
37
law of definite proportion
a given compound always contains exactly the same proportion of elements by mass (Joseph Proust)
38
law of multiple proportions
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
Dalton's Atomic Theory
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
Joseph Gay-Lussac
observed at the same temperature and pressure 2 volumes of H gas reacted with one volume O gas
41
Amedeo Avogadro
said at the same temperature and pressure that equal volumes of different gases contain the same number of particles
42
J.J. Thomson
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
Robert Millikan
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
radioactivity
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
Ernest Rutherford
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
protons
positive charge, equal but opposite in magnitude to electron charge
47
neutrons
have NO charge, about the same mass as a proton
48
atoms
no net charge, number of protons and electrons EQUAL
49
isotopes
atoms or ions with the same number of protons but DIFFERENT numbers of neutrons
50
atomic number (Z)
number of protons
51
Mass number (A)
sum of protons and neutrons in nucleus
52
ion
atom or group of atoms with a net positive or negative charge
53
cation
positively charged ion
54
anion
negatively charged ion
55
ionic solid (salt)
solid made of oppositely charged ions, can be simple (K+) or polyatomic (NO3-)
56
metals
tend to be conductive, malleable, lustrous and ductile elements, tend to LOSE electrons
57
non-metals
tend to be non-conductors, brittle, not lustrous, tend to GAIN electrons
58
groups/families
elements in the same vertical column
59
alkali metals
form 1+ cations
60
alkaline earth metals
form 2+ cations
61
halogens
form 1- anions
62
noble gases
usually don't like to gain or lose electrons, usually monoatomic
63
periods
elements in the same horizontal rows on the periodic table
64
mass spectrometer
used to determine atomic masses
65
Carbon-12
used as standard for all atomic masses, other masses are relative to it
66
mole
number of carbon atoms in exactly 12 grams of pure carbon-12
67
Avogadro's number
6.022 * 10^23 (atoms or molecules per mole)
68
chemical bonds
forces that hold atoms together in compounds
69
covalent bonds
sharing electrons to bond together; also called a molecule
70
empirical formula
smallest whole number ratio of elements in a compound (ex. CH3)
71
molecular formula
number and type of elements needed to represent one complete molecule of a compound (ex. C2H6)
72
structural formula
individual bonds between atoms are shown (as a line), each line also represent the 2 electrons that make up the bond
73
ball and stick model
shows atoms and their relative orientation to one another in the molecule
74
space filling model
shows the relative size of atoms and their relative orientation in a molcule
75
ionic bonds
forces of attraction between oppositely charged ions (cation + anion), usually stronger than covalent bond
76
binary compound naming rules
1) cation is first, followed by anion 2) monoatomic cation takes its name from the name of the element (ex. sodium chloride)
77
binary compound type 2
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
-ic
cation with higher charge (ex. Fe 3+ is ferric ion)
79
-ous
cation with lower charge (ex. Fe 2+ is ferrous ion)
80
transition metal charges
Ag+, Zn2+, Sc 3+, Al 3+,
81
oxyanions
anions that contain oxygen
82
binary covalent compounds
molecules formed by 2 atoms sharing valence electrons (usually 2 nonmetals), do NOT contain ions
83
binary covalent compounds naming rule
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
vowel drop rule
often the last letter of the prefix is dropped when it is followed by a vowel
85
acid naming rule
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
hydrated ionic compounds (hydrates)
ionic compounds with a specific number of water molecules associated with the formula (ex. CuSO4 * 5 H2O is sulfate pentahydrate)
87
molar mass (molecular weight)
the mass per mole of any material
88
percent composition of compounds
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
mass percentage method
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
combustion analysis
completely incinerate a sample to determine the mass of all elements present
91
reactants
on left side of arrow in chemical equation
92
products
on right hand side of arrow in chemical reaction

Chemistry 121 (6 decks)

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