Exam 1 Flashcards
What does alcohol chemicals always end in
-ol
what is chem
matter and the changes it undergoes
what is matter
has mass and takes up space
nanoscale
atoms/molecules (h2o)
macroscale
what we see in the living world (cup of water)
physical properties
measurable or observable property that does not alter the identity of the material
examples of physical properties
color, volume, freezing point, melting point, mass (weight),odor
chemical properties
describes reactivity
-identity of materials will change
examples of chemical properties
flammability, combustion
Intensive properties
do not depend on amount of material present
-melting point, freezing point,boiling point, density,color
extensive properties
depend on amount of material present
-mass, volume
reaction formula
Left: reactants Right: product
h2o(s) –> h2o(l)
physical change
occurs but does not alter identity
-water melting
chemical change
alters identity, allows bonds to break and new atom combinations to form
-combustion
what are signs of a chemical change
bubbles
color changes
new smells
new temperature
solid
lots of interactions between close packed particles, order
definite shape
definite volume
liquid
moderate interactions distance between particles varies
indefinite shape
defintie volume
H
hydrogen
He
helium
Li
lithium
Be
beryllium
B
boron
C
carbon
N
nitrogen
O
oxygen
F
flourine
Ne
neon
Na
sodum
Mg
magnesium
al
aluminum
si
silicon
p
phosphorus
s
sulfer
cl
clorine
ar
argon
k
potassium
ca
calcium
sc
scandium
ti
titanium
v
vanadium
cr
chromium
mn
manganese
fe
iron
co
cobalt
ni
nickel
cu
copper
zn
zinc
ga
gallium
ge
germanium
as
arsenic
se
selenium
br
bromine
kr
krypton
gas
large separation between particles, no interaction between particles
- indefinite shape
- indefinite volume
- -only compressible state
two principle classes of matter
- pure substance
2. mixture
two types of pure substances
- element (1 type of atom)
2. compound (2+ types of atoms bonded)
two types of Mixtures
- homogeneous - uniform throughout
2. heterogeneous - not uniform throughout
three physical processes to separate a mixture
- object selection
- filtration
- distillation
element
only one the of atom involved, cannot be broken down into something simpler
monotomic
most elements - only one atom
diatomic
7 atoms, always found with two particles
what are the 7 diatomic atoms
I2 I Br2 bring Cl2 clay F2 for O2 our N2 new H2 home
Compound
chemical combination of 2+ elements
- atoms bonded together into a single unit
- makes a molecule
mixture
physical combination of 2+ pure substances
-all pure substances in mixture retain their own chemical identity
homogeneous mixture
evenly distributed throughout
-aka a solution
mixtures of gas are always….
homogeneous
heterogeneous mixture
top does not equal bottom
yours does not equal mine
mass
kilogram
length
meter
time
second
temp
kelvin
amount of a substance
mole
giga
10^9
mega
10^6
kilo
10^3
deci
10^-1
centi
10^-2
milli
10^-3
micro
10^-6
nano
10^-9
Conversion factor
relates two units
ie $1 = 4 quarters
dimensional analysis/stolchiometry
setting up math to allow for unit conversions
who proposed the atomic theory based on four postuates
John Dalton
Four postulates
- each element is composed of extremely small particles called atoms
- each element has it’s own kind of atom - all atoms of a given element are identical in mass and properties
- physical and chemical - atoms are neither created nor destroyed during chemical reactions, and atoms of one element cannot be changed into atoms of another element
- atoms from different elements can combine to form compounds
- oxygen+nitrogen=nitrogen monoxide (forms molecule)
what did daltons atomic theory explain
- the law of constant composition
- the law of conservation of mass
- the law of multiple conversions
the law of multiple conversions
if two elements combine to form more than one product the atoms will combine in whole number ratios
- compounds possible when carbon combines w oxygen CO and CO2
- -12g C + 16g O = CO
- -12g C + 32 g O = CO2
JJ Thompson
cathode ray tube
- beam of light goes from cathode (-) to anode (+) and when (+) magnet is put behind it light attracts, when (-) magnet is put behind it light deflects
- -beam is a beam of eelectrons
Millikan
oil drop
Isotope
Forms of an element with same number of protons but different number of neutrons
Atomic weight formula
Sum of all (isotope)(abundance as decimal)
H atomic weight
(1H mass)(abundance)+(2h mass)(abundance)+(3h mass)(abundance)
Molecules
A collection of non metal atoms
All atoms must be found on right side of staircase and hydrogen
Covalent bond
Between atoms that share electrons
Can be single, double, or triple
Between a nonmetal & non metal
Naming of covalent bonds
Based on number of each specific atom in compound, Must use prefix Mono Di Tri Tetra Penta
Metal atoms in an ionic compound
Lose electrons
-positive: cation
Non mental atoms in an ionic compound
Gain electrons
-negative: anion
How to name ionic compound
Cation (metal), anion (non metal
How are ionic bonds connected
Stuck together by electrostatic attraction
Exceptions of ions
NH4+ polyatomic cation ammonium
NH4Cl ionic
H+
hydrogen ion
Li+
litium ion
Na+
sodium ion
K+
potassium ion
Cs+
cesium ion
Ag+
silver ion
Mg2+
magnesium ion
Ca2+
calcium ion
Sr2+
strontium ion
Ba2+
barium ion
Zn2+
zinc ion
Cd2+
Cadmium ion
Al3+
aluminum ion
NH4+
ammonium ion
Cu+
copper(I) or Cuprous ion
Co2+
cobalt(II) or cobaltous ion
Cu2+
copper (II) or cupric ion
Fe2+
iron (II) or ferrous ion
Mn2+
Maganese(II) or manganous ion
Hg2^2+
mercury (I) or mercurous ion
Hg^2+
mercury(II) or mercuric ion
Ni2+
Nickel(II) or nickels ion
Pb2+
lead(II) or plumbous ion
Sn2+
Tin(II) or stannous ion
Cr3+
chromium(III) or chromatic ion
Fe3+
Iron(III) or ferric ion
H-
Hydride ion
F-
floride ion
Cl-
chloride ion
Br-
bromide ion
I-
iodide ion
Cn-
cynide ion
OH-
Hydroxide ion
O^2-
oxide ion
O2^2-
peroxide ion
S2-
Sulfide ion
N3-
Nitride ion
CH3COO- (or C2H3O2-)
Acetate ion
CIO3-
Chlorate ion
CLO4-
perchlorate ion
NO3-
Nitrate ion
MnO4-
permanganate ion
CO3^-2
carbonate ion
CrO4^-2
dichromate ion
SO4^-2
sulfate ion
PO4^-3
Phosphate ion
polyatomic ions
group of atoms covalently bonded together BUT has a charge
—–NH4+
oxyanions w/o halogens
More molecules of O: -ate
Less molecules of O: -ide
Oxyanions w/ halogen
4 per-__-ate
3 -ate
2 -ite
1 hypo-___-ite
How to balance reactions
coefficients
Aqueous solution
salt disolved in water
metal+non metal=
salt! which contains ions, so make ions first
Combustion reaction
Involved compounds hydrocarbons organic hydrocarbons (H,C,O)
Burn in o2, burn in “air” only o2 involved
Hydrocarbon + o2
CO2(g)+H2O(g)+heat
Formula weight
Sum of atomic weights of atoms present in formula unit
-ions (salts)
Molecular weight
Sum of atomic weights of atoms present in molecule
-covalent bond (molecules)
At room temperature ionic bonds/salts are always
Solid crystal
Percent composition
Tells you what portion of the entire mass of a substance is due to a specific type of atom
Atom amu/total amu x100%
1 mole/Avogadros number
Collection of 6.02x10^23 items
-only ever items you can’t see
