 | Term | Definition |
| |
measurement |
quantity with both number and unit |
| |
scientific notation |
an expression of numebers in the form m x 10^x where m is equal to or grater than one and less than ten, and n is an integer |
| |
accuracy |
a measure of how close a measurement comes to the actual or true value of whatever is measured |
| |
precision |
measure of how close a series of measurements are to one another |
| |
accepted value |
correct value based on reliable references |
| |
experimental value |
value measured in the lab |
| |
error |
experimental value-accepted value |
| |
percent error |
absolute value of the error divided by the accepted value, multiplied by 100\ |
| |
significant figure |
include all of the digits that are known + a last digit that is estimated. |
| |
non zero digit |
assumed to be significant |
| |
zeros between non zero digits |
significant |
| |
leftmost zeros |
not significant |
| |
zeros at the end of a number and to the right of a decimal point |
always significant |
| |
five S.I. base units |
meter, kilogram, kelvin, second, mole |
| |
gram |
1/1000 of a kilogram |
| |
Celsius freezing point |
0 degrees |
| |
Celsius boiling point |
100 degrees |
| |
Kelvin freezing point |
273.15 |
| |
Kelvin boiling point |
373.15 |
| |
The zero point on Kelvin Scale |
absolute zero |
| |
Celsuis to Kelvin |
C + 273 |
| |
Kelvin to Celsius |
K - 273 |
| |
cm in meters |
100 centimeters in a meter |
| |
grams to kilograms |
1000 grams in a kilogram |
| |
valence electrons |
electrons in highest occupied energy level |
| |
number of valence electrons |
group number |
| |
cation |
positive ion |
| |
anion |
negative ion |
| |
ionic bonds |
electrostatic forces that hold ions together in ionic compounds |
| |
chemical formula |
shows the kinds and numbers of atoms in the smallest representative unit of a substance |
| |
formula unit |
lowest whole number ratio of ions in an ionic compound |
| |
ionic compounds |
crystalline solids at room temperature and high melting points |
| |
coordination number |
the number of ions of opposite charge that surround the ion in a crystal |
| |
ionic compound conductivity |
electric current when melted or dissolved in water |
| |
sea of electrons |
model of valence electrons |
| |
metallic bonds |
consist of the attraction of the free floating valence electrons for the positively charged metal ions |
| |
alloy |
mixture composed of two or more elements; at least one is a metal |
| |
covalent bond |
a bond formed by the sharing of electrons between atoms |
| |
molecule |
neutral group of atoms joined by covalent bond |
| |
molecular formula |
chemical formula of a molecular compound |
| |
type of configuration wanted by electrons |
noble gas |
| |
structural formula |
represents the covalent bonds by dashes and shows the arrangement of covalently bonded atoms |
| |
unshared pair |
pair of electrons not shared between atoms |
| |
coordinate covalent bond |
covalent bond in which one atom contributes both bonding electrons |
| |
polyatomic ion |
tightly bond group of atoms that has a positive or negative and behaves as a unit |
| |
bond dissociation energy |
the energy required to break the bond between two covalently bonded atoms |
| |
resonance structure |
a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecue or ion. |
| |
non polar covalent bond |
a covalent bond in which the electrons are shared equally |
| |
polar covalent bond |
a covalent bond in which the electrons are not shared equally |
| |
Vanderwaals Forces |
the two weakest attractions between molecules |
| |
dipole interactions |
occur when polar molecule are attracted to one another |
| |
dispersion forces |
weakest of all molecular attractions and caused by motion of electrons |
| |
hydrogen bonds |
attactrative forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared pair of another electronegative atom |
| |
network solid |
solids in which all of the atoms are covalently bonded together |
| |
binary compound |
composed of 2 elements and can be ionic or molecular |
| |
naming ionic binary compound |
cation name first, then anion name |
| |
acid |
compound that contains one or more hydrogen atoms and produces hydrogen ions when dissolved in water |
| |
name of anion - ide |
acid name begins prefiz hydro, and suffix ic followed by acid |
| |
anion ending in ite |
stem of anion with suffix ous followed by acid |
| |
anion ending in ate |
stem of anion with suffix ic followed by acid |
| |
base |
ionic compound that produces hydroxide ions when dissolved in water |
| |
mole |
6.02 x 10^ 23 |
| |
another name for mole |
avogadro's number |
| |
representative particle |
refers to the species present in a substance (atom, molecule, or formula unit) |
| |
number of particles to mole |
representative particles x one mole/ 6.02 x 10^23 |
| |
moles to number of particles |
mole x 6.02 x 10^23/ one mole |
| |
molar mass |
a term used to refer to the mass of a mole of any substance (g/mole) |
| |
writing word equations |
names of reactants to the left of the arrow separated by + signs; write the names of the products to the right of the arrow also separated by + signs |
| |
chemical equation |
representation of a chemical reaction |
| |
skeleton equation |
a chemical equation that does not indicate the relative amounts of the reactants and products |
| |
catalyst |
a substance that speeds up the reaction but is not used in the reaction |
| |
coefficients |
small whole numbers that are placed in front of the formulas in a equation in order to balance it. |
| |
balanced equation |
a chemical equation in which mass in conserved; each side of the equation has the same number of atoms of each element |
| |
five general types of reactions |
combination, decomposition, single-replacement, double-replacement, and combustion |
| |
combination reaction |
chemical change in which two or more substances react to form a single new substance |
| |
group A metal + non metal |
product is a compound consisting of the metal cation and the non metal anion |
| |
two non metals react |
more than one product is often possible |
| |
decomposition reaction |
chemical change in which a single compound breaks down into two or more simpler products |
| |
single replacement reaction |
chemical change in which one element replaces a second element in a compound |
| |
activity series |
lists metals in order of decreasing reactivity |
| |
double replacement reaction |
a chemical change that involves an exchange of positive ions between two compounds |
| |
combustion reaction |
a chemical change in which an element or compound reacts with oxygen, often producing energy in the form of heat and light |
