Chemistry Honors Flashcards
Charles’ law
V1/T1 = V2/T2
Volume and temperature are inversely related
Pressure Conversions
1atm= 760. mm HG= 760 torr = 101.3 kpa = 14.7 psi
Boyle’s Law
P1V1= P2V2
As pressure increases, volume increases
Combine gas law
P1V1/ T1= P2V2/T2
Gay-Lussac Law
P1/T1= P2/T2
Ideal Gas Law
PV=NRT
Proton
A subatomic particle having a single positive electric charge.
Equal to atomic number.
Neutron
Subatomic particles with a neutral charge
Electron
Subatomic particle that has a very low mass and carries a single negative electric charge
Mass number
The total number of neutrons and protons present in the nucleus of an atom.
Atomic number
Number of protons in the nucleus
Ions
An atom or group of atoms that has a net positive or negative charge.
Isotopes
Atoms having the same atomic number but different mass numbers.
Symbols
One or two letters used to represent the names of elements. The first letter is always capitalized
Ex: Co is cobalt
Hg is mercury
Homogenous mixture
A mixture that has the same composition throughout.
Ex: salt water
Sugar water
Heterogeneous mixture
A mixture in which the composition is not uniform
Ex: oil and waters
Sand and iron
To convert Fahrenheit to Celsius…
C= (F-32) x 5/9
To convert Celsius to Fahrenheit
F= 9/5 (C + 32)
Convert from Celsius to Kelvin
K=C + 273.15
1 in = ? cm
2.54
1 lb= ? G
453.6 g
1qt= ? mL
946 mL
1 mile= ?ft
5280 ft
1000 m= ? Km
1 km
Significant figures
If there is a decimal, move from left to right and start with the first non zero number. Every number after that will be the amount of sig figs.
If there is no decimal move from right to left and start with the first non zero number and every number that comes after is sig figs.
Density
D= m/v
Ex:
1 D = ? M=2.54. V= .382 mL
D= 2.54/.382
D= 6.65 g/cm3
Physical change
Does not alter the composition or identity of a substance
Examples: sugar dissolving in water.
Breaking a pencil or paper
Chemical Change
Alters composition or identity of a substance
Examples: burning wood
Hydrogen burns in air to form water.
What are the seven families of the periodic table?
Alkali metals Alkaline earth metals Transition metals Halogens Noble gases Lanthanides Actinides
Compounds
A substance composed of two or more elements chemically united to fixed proportions.
Ex: CO2
H2O
Elements
A substance that cannot be separated into simpler substances by chemical means.
Ex: oxygen
Iron
Ionic Compound
Any neutral compound containing cations and anions
Ex: Na2SO4
MgCO3
Covalent compounds
Compounds containing only covalent bonds.
(Covalent bonds= a bond in which two electrons are shared by two atoms)
Ex:
S2CL4 (disulfur tetrachloride)
H2O6 (dihydrogen hexoxide)
Acids
A substance that yields hydrogen ions (H+) when dissolved in water.
Ex:
HCL Hydrochloric acid (binary acid)
H3PO4 phosphoric acid (ternary acid)
Bases
A substance that yields hydroxide ions (OH -) when dissolved in water
Ex:
NaOH
Polyatomic ions
An ion that contains more than one atom
No3-
Nitrate
Sulfate
SO4 -2
Carbonate
CO3 -2
Acetate
C2H3O2
ClO3 -1
Chlorate
CrO3 -1
Chromate
Atoms
The basic unit of an element that can enter into chemical combination
Molar mass
The mass in grams or kilograms of 1 mole of atoms, molecules or other particles.
Atomic mass
The mass of an atom in atomic mass units
Molecular mass
The sum of the atomic weights of the atoms in the empirical formula of the compound
Formula mass
The sum of the atomic weights of the atoms in the empirical formula of the compound.
Molarity
The molar concentration or the number of moles per solute per liter of solution.
Mass spectrometry
An analytical technique that produces spectra (singular- spectrum) of the masses of the atoms or molecules comprising a sample of material.
How does mass spectrometry work?
It works by ionizing chemical compounds to generate charged molecules or mole fragments and measuring their mass to charge ratios.
Limiting reactants
Substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reagent since the reaction cannot proceed further without it.
Theoretical yield
Amount of product that would react if all the limiting reagent reacted.
Empirical formula
Tells us which elements are present and the simplest whole number ratio of their atoms. Simplest chemical formula, must be whole numbers.
Actual yield
The amount of product actually obtained from a reaction.
Almost always less than the theoretical yield
Theoretical yield
The amount of product that would result if all the limiting reagent reacted.
It is the maximum obtainable yield predicted by the balance equation
Percent yield formula
% yield= actual yield/theoretical yield x 100%
Molecular formula
An expression showing the exact number of atoms of each element in a molecule.
To calculate the actual molecular formula, we must know its approximate molar mass and it’s empirical formula.
Percent composition
The percent by mass of each element in a compound.
Percent composition formula
((N x molar mass of element) / (molar mass of compound)) x 100
