William Deese Chem 100 Exam 1-LA Tech

matter

anything that has mass and takes up space

pure substance

A substance made of only one kind of matter and having definite properties.

mixture

A combination of two or more substances that are not chemically combined

homogenous mixture

a mixture in which the composition is uniform throughout

heterogenous mixture

A mixture with uneven distribution of different substances, solids, liquids, gases.

metals

Elements that are good conductors of electric current and heat.

nonmetals

Elements that are poor conductors of heat and electric current

metalloids

Elements that have properties of both metals and nonmetals.

physical change

A change in a substance that does not involve a change in the identity of the substance

chemical change

A change that occurs when one or more substances change into entirely new substances with different properties.

boiling point of water in celsius

100 degrees

boiling point of water in kelvin

373 K

boiling point of water in fahrenheit

212 degrees

fahrenheit to celsius

5/9(F-32)

celsius to fahrenheit

9/5 (C+32)

kelvin to celsius

K-273

celsius to kelvin

C+273

mass/volume

equation for density

unit of length

meter

kilogram

unit of mass

second

unit of time

ampere

units of electric current

kelvin/degrees

units of temperature

mole

amount of substance

candela

luminous intensity

tera (T)

10^12

giga (G)

10^9

mega (M)

10^6

kilo (k)

10^3

deci (d)

10^-1

centi (c)

10^-2

milli (m)

10^-3

micro (M)

10^-6

nano (n)

10^-9

pico (p)

10^-12

2.54 cm

1 in

1 cm^3

1 mL

significant figure

the number of all known digits reported in measurements plus one estimated digit

law of conservation of mass

Matter is neither created nor destroyed

law of definite proportions

a given compound always contains exactly the same proportion of elements by mass

atomic theory

a theory that states that all matter is composed of tiny particles called atoms.

John Dalton, 1803

who invented atomic theory and when?

Law of Multiple Proportions

if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

chadwick

Shot alpha rays at beryllium which then emmitted gamma rays; the gamma rays were a stream of neutrons, discovered the neutron

Proust

separated water into separate hydrogen and oxygen atoms-came up with law of definite proportions

millikan

Oil Drop Experiment, determined mass and magnitude of the electron

thomson

discovered the electron and raisin pudding model of an atom

rutherford

Gold foil experiment, discovered nucleus and nucleic model of an atom

Radioactivity

The process in which some substances spontaneously emit radiation waves (alpha, beta, gamma)

alpha waves

attracted by negative charges

beta waves

attracted by positive charges

gamma waves

attracted by neutral charges

proton

positive charge

neutron

no charge

electron

negative charge

marie curie

suggested the name of radioactivity

ion

An atom or group of atoms that has a positive or negative charge.

atomic number

the number of protons in the nucleus of an atom, measured in AMU (atomic mass units)

mass number

the total number of protons and neutrons in the nucleus of an atom

nucleotides

protons and neutrons together in an atom

isotope

Atoms of the same element that have different numbers of neutrons

carbon 14

a radioactive isotope of carbon used for carbon dating

period

horizontal row in the periodic table

group

Vertical column in the periodic table

alkali metals

any metal in Group 1A of the periodic table

alkaline earth metals

the elements in Group 2A of the periodic table

noble gases

elements in group 18 of the periodic table

halogens

the elements in group 17 of the periodic table

chalcogens

Elements in group 16 on the periodic table

transition metals

Elements in groups 3-12 on the periodic table

main group metals

elements in Groups 1, 2, 13-18 on the periodic table

lanthonides

top of bottom 2 rows on periodic table

actinides

bottom of bottom 2 rows on periodic table

Demitri Mendeleev

russian scientist who created periodic table

cation

A positively charged ion

monatomic ion

a single atom with a positive or negative charge

anion

A negatively charged ion

NH4+

Ammonium

OH-

Hydroxide

HSO4-

Hydrogen Sulfate

ClO-

Hypochlorite

ClO2-

Chlorite

ClO3-

Chlorate

ClO4-

Perchlorate

NO2-

Nitrite

NO3-

Nitrate

MnO4-

Permanganate

H2PO4-

dihydrogen phosphate

CN-

Cyanide

HCO3-

Hydrogen Carbonate

CO3^2-

Carbonate

HPO4^2-

hydrogen phosphate

Cr2O7^2-

Dichromate

S2O3^2-

Thiosulfate

SO3^2-

Sulfite

SO4^2-

Sulfate

C2O4^2-

Oxalate

PO4^3-

Phosphate

H3O+

Hydronium

CrO4^2-

Chromate