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mass
measure of the resistance of an object to a change in its state of motion
weight
force extended by gravity on an object
deci
.1
centi
.01
mili
.001
1dm³
1000 cm³
1cm³
1 mL
law
statement of observed behavior
theory
attempt to explain why something happens
natural law
observed measurable behavior
steps of scientific method
make observations, formulate hypothesis, perform experiments
accuracy
agreement of a particular value with the true value
precision
degree of agreement among several measurements of the same quantity
(sig figs) Non zero digits
always sig fig
(sig figs) leading zeros
never sig fig
(sig figs) captive zeros
always sig fig
(sig figs) trailing zeros
only sig fig if the number has a decimal point
(sig figs) exact numbers
infinite number of sig figs
sig fig rules for addition or subtraction
result has same number of decimal places as the least precise measurement in equation
sig fig rules for multiplication or division
result has the same amount of sig figs as the least precise measurement in the equation
density
d=m/v
matter
anything that has weight and takes up space
homogenous mixture
parts cannot be seen
heterogenous mixture
parts can be seen
properties of a solid
rigid, fixed volume and shape, slightly compressible
properties of a liquid
definite volume, no specific shape, slightly compressible
properties of a gas
no fixed volume or shape, highly compressible
mixture
has variable composition, can be separated into pure substances, behaves the same as before they were mixed and after being separated
physical change
change in form, no change in chemical substance, used to separate mixture into compounds
3 methods of separating components in a mixture
distillation, filtration, chromatography
distillation
depends on boiling point, heating the mixture, vapor is passed through condenser where it returns to liquid state
filtration
used when mixture contains a solid and a liquid; liquid passes through filter, solid stays behind
chromatography
mobile phase, stationary phase; separation occurs because the components have different affinities for the two phases
compound
pure substance with a constant composition that can be broken down into its elements
element
pure substance that cannot be further broken down by physical or chemical means
law of multiple proportions
when two elements form a series of compounds, the ratios of the masses of the second element that combine with the 1g of the first elements can always be reduced to small whole numbers
dalton’s atomic theory
each element is made up of atoms, atoms of any given element are identical, chemical compounds are formed when atoms of two elements combine, chemical reactions involve the reorganization of atoms
cathode ray
cathode ray was a stream of electrons
radioactivity
discovered through spontaneous emission by uranium
gamma rays
high energy light
beta particles
high speed electrons
alpha particles
particles with 2+ charge
protons
positive charge, in the nucleus of the atom, amount determines the element
electron
negative charge, in the electron cloud around the nucleus of the atom
isotope
atoms with the same number of protons but different numbers of neutrons
covalent bond
sharing of electrons
chemical formula
uses symbols of elements to indicate types of atoms present in the molecule, subscripts indicate relative number of atoms
ion
atom or group of atoms with a negative or positive charge
cation
positive ion formed by losing electrons
anion
negative ion formed by gaining electrons
ionic bond
force of attraction between oppositely charged ions
alkali metals
Grp 1A, lose 1e to form 1+ ion
alkali earth metals
grp 2A, loses 2e to form 2+ ion
halogens
grp7A, form diatomic molecules
noble gases
grp8A, normal conditions under monatomic gases, little chemical reactivity
Diatomic Elements
HOFBrINCl (hydrogen, oxygen, fluorine, bromine, iodine, nitrogen, chlorine)
binary compounds
composed of 2 elements, some include covalent and ionic compounds
binary ionic compounds
contain a cation (written first), and an anion
type of compound if compound starts with a metal or polyatomic
ionic
type of compound if compound starts with nonmetal
moelcular/covalent
type of compound if compound starts with H
acid (except water)
grp 1A form charge
1+
grp 2A form charge
2+
Al charge
3+
Ag charge
+
Zn charge
2+
Cr, Mn, Fe, Co charges
2+ or 3+
Cu charges
2+ or +
Cd charge
2+
Sn and Pb charges
2+ or 4+
naming polyatomic ions
use prefix hypo- to name members in series with fewest O atoms, use prefix per- to name members with most O atoms
OH-
hydroxide
NO3
nitrate
SO4
sulfate
NH4+
ammonium
PO4³-
phosphate
C2H3O2
acetate
CO3²-
carbonate
binary covalent
between 2 nonmetals, name with prefixes
Naming Acids
depends on whether O is present; if anion ends in -ide - prefix hydro and sufficx-ic; anion contains O - root name of anion suffix -ic (ate) or -ous (ite)
formula F to C
(F-32)5/9
formula C to F
(Cx9/5)+32
formula K to C
C + 273.15
formula C to K
K - 273.15
results of rutherford
atoms is mostly open space with a dense nucleus
results of milikan
determined that all electrons are the same in mass and charge
results of thomson
determined that electrons are negative