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Chemistry Midterm Review
N/A
107
Chemistry
11th Grade
01/12/2015

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Term
Mass
Definition
Quantity of matter in an object
SI base unit: kg
Term
volume
Definition
space that an object occupies
SI base unit: mL cm3
Term
solid
Definition
fixed volume and shape; particles vibrate
Term
liquid
Definition
fixed volume but not shape; particles slip past each other.
Term
gas
Definition
no fixed volume or shape. fastest moving particles
Term
1 cm3 =
Definition
1 mL
Term
1 dm3 =
Definition
1,000 mL or 1 L
Term
allotrope
Definition
one of a number of different molecular forms of an element. such as; O2-oxygen and O3-ozone
Term
formula for density
Definition
d=m/v
Term
2 groups that make up pure substances
Definition
elements and compounds
Term
law of conservation of energy
Definition
Mass of product equals the mass of the reactants
Term
Law of Conservation of Energy
Definition
The total quantity of energy remains constant. It cannot be created or destroyed.
Term
Kelvin to Celcius
Definition
-273
Term
Celcius to Kelvin
Definition
+273
Term
scientific method
Definition
Specific procedures for conducting research -make/test hypothesis
-observe
-draw conclusions
-publish results
-construct theory
Term
theory
Definition
a well-tested explanation of observations. Can be disproved but not fully proven
Term
hypothesis
Definition
a reasonable and testable explanation for observations
Term
confined zeros
Definition
significant
Term
leading zeros
Definition
not significant
Term
trailing zeros following a decimal point
Definition
significant
Term
qualitative
Definition
describing something with properties such as texture and color used to describe quality
Term
quanttative
Definition
describing something with numbers
Term
chemical change
Definition
identity changes. new substance forms
-evolution of gas
-precipitate forms
-release(exothermic) or absorption(endothermic) of energy
-color change
Term
physical change
Definition
identity does not change. can change state/mix but remain the original substance
Term
law of definite proportions
Definition
two samples of a given compound are made of the same elements in the proportions by mass regardless of the sizes of sources of the samples
Term
law of multiple proportions
Definition
if two or more different compounds are composed of the same elements, the ratio of mass in the second one is always a ratio of small whole numbers
Term
Daltons theory
1(revised)
Definition
all matter is composed of extrememly small particles called atoms that cannot be subdivided or destroyed
Term
Daltons theory
2 (revised)
Definition
Atoms of a given element are identical in their physical and chemical properties
Term
Daltons theory
3
Definition
Atoms of different elements differ in their physical and chemical properties
Term
Daltons theory
4
Definition
Atoms of different elements combine in simple, whole-number ratios to form compounds
Term
Daltons theory
5
Definition
In chemical reactions, atoms are combined, rearranged, or separated but NEVER created or destroyed.
Term
which subatomic particles reside in the nucleus?
Definition
protons-positive
neutrons- no charge
Term
subatomic particle outside the nucleus
Definition
electrons- negative
Term
isotope
Definition
Atoms of the same element with a different number of NEUTRONS
Term
ion
Definition
an atom, radical or molecule that has gained or lost one or more electrons and now has a neg or pos charge
Term
what happens when an electron gains energy
Definition
it moves into an excited state
Term
returning from an excited to ground
Definition
it releases a specific quantity of energy and quickly falls back to its ground state
Term
Principal quantum number (n)
Definition
indicates main level energy occupied by the electron ~1,2,3,4
Term
Angular quantum number (l)
Definition
indicates the shape or type of orbital that corresponds to a particular sublevel
=0(s);
=1(p);
=2(d);
=3(f)
Term
Magnetic Quantum Number (m)
Definition
is a subset of the L quantum number. indicates the number/orientations around the nucleus
1-s orbital
3-p orbitals
5-d orbitals
7-f orbitals
Term
orbitals/electrons in s
Definition
1 orbital; 2 e-
Term
orbitals/electrons in p
Definition
3 orbitals; 6 electrons
Term
orbitals/electrons in d
Definition
5 orbitals; 10 e-
Term
orbitals/electrons in f
Definition
7 orbitals; 14 e-
Term
aufbau
Definition
"building up"
e- fill orbitals with lower energy first
s>p>d>f
Term
Hund's
Definition
orbitals of the same n and L quantum numbers are each occupied by one before paring occurs
Term
Pauli
Definition
two particles of a certain class cannot be in the exact same energy state ^^ or vv
Term
Periodic Law
Definition
The physical or chemical properties tend to repeat systematically with increasing atomic number
Term
4f
Definition
lanthanide
Term
5f
Definition
actinide
Term
4f or 5f radioactive?
Definition
5f- actinides
Term
malleable
Definition
can be hammered into a sheet and remain conductive
Term
ductie
Definition
can be stretched into thin wire and remain conductive
Term
electron sheilding
Definition
outer, valence e- held less tightly to nucleus
Term
down a group, e- shielding
Definition
atomic radius increases down a group
Term
as the nuclear charge increases across a period
Definition
the effective nuclear charge also increases
Term
ionization energy
Definition
the amount of energy needed to remove an electron from an atom
Term
ionization energy
-decreases
-increases
Definition
ionization energy
-down a group
-across a period
Term
electronegativity
Definition
a measure of the ability of an atom in a chemical COMPOUND to attract electron
Term
electronegativity
-decreases
-increases
Definition
electronegativity
-down a group
-across a period
Term
electron affinity
Definition
the change in energy when a neutral atom gains an electron
Term
electron affinity
-decreases
-increases
Definition
electron affinity
-down a group
-across a period
Term
ionic radii
-increases
-decreases
Definition
ionic radii
-down a group
-across a period
Term
atomic radii
-increases
-decreases
Definition
atomic radii
-down a group
-across a period
Term
group 1
Definition
1+
Term
group 2
Definition
2+
Term
group 15
Definition
3-
Term
group 16
Definition
2-
Term
anion
Definition
ion with a negative charge
Term
cation
Definition
an ion with a positive charge
Term
common between an ion and its parent atom
Definition
proton count
Term
lattice energy
Definition
the amount of energy released when an ionic bond is formed
Term
bond energy
Definition
energy required to break the bond of 1 mole of a chemical compound
Term
properties of ionic compounds
Definition
-hard and brittle
-good conductors
-strong
-high boiling and melting points
-solid at room temp
Term
for an ionic compound to conduct
Definition
-substance must contain charged particles
-must be free to move
Term
strongest attractive forces
Definition
ionic
Term
why are ionic compounds considered brittle?
Definition
when you apply a strong force, fracture occur, not dents
Term
CH3COO(1-)
Definition
acetate
Term
S2O3(2-)
Definition
thiosulfate
Term
NO2(1-)
Definition
nitrite
Term
NO3(1-)
Definition
nitrate
Term
PO4(3-)
Definition
phosphate
Term
CO3(2-)
Definition
Carbonate
Term
CN(1-)
Definition
cyanide
Term
CrO4(2-)
Definition
Chromate
Term
SO4(2-)
Definition
Sulfate
Term
SO3(2-)
Definition
Sulfite
Term
OH(1-)
Definition
Hydroxide
Term
MnO4(1-)
Definition
Permaganate
Term
Cr2O7(2-)
Definition
Dichromate
Term
NH4(2-)
Definition
Ammonium
Term
Covalent Bond stronger/weaker than ionic
Definition
weaker than ionic
Term
weakest type of covalent bond
Definition
nonpolar covalent
Term
tetrahedral
atoms:
bonds:
Definition
tetrahedral
5
4
Term
0-0.5
Definition
nonpolar
Term
.6-2.0
Definition
polar covalent
Term
2.1-4
Definition
ionic compound
Term
avogrados number
Definition
6.022x10^23
Term
molar mass
Definition
an average of the abundances of each weight of the element
Term
mass>particle
Definition
mass given| 1 mol | avogrados#
..........|molar mass|1mol
Term
particle>mass
Definition
Part. given| 1 mol | molar mass
.........|avorgado#| 1 mol
Term
1A
Definition
alkali
Term
2A
Definition
alkaline earth
Term
17A
Definition
halogens
Term
18
Definition
noble gases
Term
3-12
Definition
transition metals (d block)
Term
which in d block break Aufbau to become more stable?
Definition
Cromium and Copper
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