CHEM111 PRELIM REVIEWER Flashcards
field of study concerned with the characteristics, composition, and transformations of matter
chemistry
Icludes all things, both living and nonliving.
matter
2 types of property
physical , chemical
characteristics that can be observed without changing the basic identity of the substance
physical property
Color, odor, physical state, melting/boiling point, hardness
physical property
describes the way the substance undergoes or resists change to form a new substance
chemical property
changes its physical appearance but not is chemical composition
physical change
substance undergoes a change in chemical composition. It always involve conversion of the material under consideration into one or more new substances.
chemical change
composition of a substance does not change
physical
properties observable without changing composition
physical properties
changes observable without changing composition
physical change
changes in color, shape , solid, liquid, gas, boiling point, melting point
physical properties
melting, boiling, freezing
physical change
changes in state of subdivision with no change in state
physical change
properties that describe how a substance changes or resist change to form a new substance
chemical properties
flammability
chemical properties
decomposition, reaction to chlorine
chemical properties
changes in which one or more new substance are formed
chemical change
2 classes of matter
pure substance, mixtures
2 sub of pure substances
elements and compounds
2 types of mixtures
homo heterogenous
2 chemical composition as a_______
pure substance, mixture
CC single kind of matter that cannot be separated into other kinds of matter by any physical means
Pure Substance
CC physical combination of two or more pure substances in which each substance retains its own chemical identity
Mixture
CC components can be separated using physical means
mixture
mixture that contains visible different phases (parts), each of which has different property
hetero
contains only one visibly distinct phase
homo
pure substance that cannot be broken down into simpler pure substances by chemical means
element
pure substance that can broken down into two or more simpler pure substances by chemical means
compound
how many known elements in the PT
117
smallest particle of an element that can exist and still have the properties of the element
atom
rarely encountered in nature
free atoms
a group of two or more atoms that functions a unit because the atoms are tightly bound together
molecule
molecule that contains two atoms
diatomic molecule
`molecule that contains 3 atoms
triatomic molecule
molecule in which all atoms present are of the same kind.
e.g H2
homoatomic molecule
molecule in which two or more kinds of atoms are present.
H20
heteroatomic molecule
molecules made of atoms from different elements
compound
atoms connected by chemical bond
molecules
T/F
ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS
TRUE
notation made up of the chemical symbols of the elements present in a compound and numerical subscripts (located to the right of each chemical symbol) that indicate the number of atoms of each element present in a molecule of the compound.
CHEMICAL FORMULA
determination of the dimensions, capacity, quantity, or extent of something
MEASUREMENT
two systems of measurement that is used commonly
the English system of units and the metric system of units
inch, foot, pound, quart, and gallon
English
gram, meter, and liter
Metric
1 m is equivalent to —yards
1.09 yards
28 g =
1 ounce
454 g=
1 pound
1 L is equivalent to
1,06 quarts
T/F
Measurements will always have a degree of uncertainty or error
T
in a measurement that are known with certainty plus one digit that is estimated
SIGNIFICANT FIGURES
Number of significant figures = all certain digits + one estimated digit
YES
T/F
All nonzero digits are NOT significant
F
T/F
Zeros may or may not be significant
T
Zeros at the beginning of a number are never significant
T
Zeros between nonzero digits are always significant
T
Zeros at the end of a number are SIGNIFICANT if a decimal point is PRESENT in the number
T
Zeros at the end of a number are NOT SIGNIFICANT in the number LACKS an explicitly shown decimal point
T
0.0141
3
3.063
4
100
1
100.
3
0.001004
4
56.00
4
0.05050
4
6010
3
ratio that specifies how one unit of measurement is related to another unit of measurement
conversion factor
a general problem-solving method in which the units associated with numbers are used as a guide in setting up calculations
dimensional analysis
ratio of the mass of an object to the volume occupied by that object
density
density triangle
M/dv
indicator of the tendency of heat energy to be transferred
temp
All matter is made up of small particles called
atoms
Atoms, in turn, are made up of even smaller particles
subatomic particle
Three types of subatomic particles
protons neutrons electrons
where does the p an n located
center
the outer region contain
all electron
any subatomic particle found in the nucleus of an atom
nucleon
An atom as a whole is electrically —–
neutral
the number of protons in the nucleus of an atom
atomic number
number of protons =
number of electrons
The mass number is the number of
protons and the number of neutrons in the nucleus
number of protons + number of neutrons
mass number
An atom must have the same number of electrons and protons
yes
t/f
However, the number of neutrons do not have to be the same as the number of protons or electrons
t
atoms of an element that have the same number of protons and the same number of electrons but different numbers of neutrons
isotopes
the calculated average mass for the isotopes of an element, expressed on a scale where 126C serves as the reference point
atomic mass
states that when increasing atomic number, elements with similar chemical properties occur in periodic (regularly recurring) intervals
pt law
a tabular arrangement of the elements in order of increasing atomic number such that elements having similar chemical properties are positioned in vertical columns
pt
horizontal row of elements in the periodic table
period
vertical column of elements in the periodic table
group
Four Groups of elements have common (non-numerical) names
Alkali metal, Alkaline earth metal, Halogen and Noble Gas
an element that has the characteristic properties of luster, thermal conductivity, electrical conductivity, and malleability
metal
an element characterized by the absence of properties of luster, thermal conductivity, electrical conductivity, and malleability
nonmetal
The majority of the elements are
metals
region of space about a nucleus that contains electrons that gave approximate the same energy and that spend most of their time approximately the same distance from the nucleus
electron shell
region of space within an electron shell that contains electrons that have the same energy
electron subshell
region of space within an electron subshell where an electron with a specific energy is most likely to be found
electron orbital
spherical in shape
s
have shaped similar to the “figure 8”
p
clover shape
d
pompoms
f
electron in the outermost electron shell of a representative or noble-gas element
valence electron
the chemical symbol of an element surrounded by dots equal in number to the number of valence electrons present in atoms of the element
The general practice in writing
lewis symbol
If an atom gains one or more electrons
it becomes a negatively charged ;
if an atom loses one or more electrons,
it becomes a positively charged
ionic bond model
+1,2,3 -1,23
Ionic compounds are always
NEUTRAL
Ionic bonds form between atoms of
dissimilar elements (metal + nonmetal).
Covalent bond occurs between
similar or even identical atoms (often two nonmetals are involved)
Ionic bond =
ELECTRON TRANSFER
Covalent bond =
Electron sharing
written statement that uses chemical symbols and chemical formulas instead of words to describe the changes that occur in a chemical reaction
chemical equation
written on the left side of equation,
Reactants
written on the right side of equation,
Product
a process in which at least one new substance is produced as a result of chemical change
chemical reaction
a reaction in which a single product is produced from two (or more) reactants
combination reaction
a chemical reaction in which a single reactant is converted into two (or more) simpler substances (elements or compounds
decomposition reaction
chemical reaction in which an atom or molecule replaces an atom or group of atoms from a compound
single-replacement
a chemical reaction in which two substance exchange parts with one another and form two different substances
double-replacement
a chemical reaction between a substance and oxygen (usually from air) that proceeds with the evolution of heat and light (usually from a flame)
combustion reaction
ounce to g
23 g
lb to g
454 g
l to quarts
1.06 quarts
inch to cm
2.54 cm
m to in
39.4 in
km to mile
o.621 mile
kg to lb
2.20 lb
oz to g
28.3 g
quart to liter
0.946 liter
liter to gallon
0.265
ml to fl oz
0.038
