Chemistry Semester One

Based off of Maya's exam review

law of conservation of matter and energy

states that matter and energy can neither be created or destroyed

solid

closely packed together and contain the least amount of kinetic energy.

definite size and shape

liquid

nearly incompressible fluid that conforms to the shape of its container but retains a constant volume independent of pressure.

gas

one of the four fundamental states of matter consisting of particles that have neither a defined volume nor shape.

matter

any substance that has mass and takes up space by having volume.

mass

measure of the amount of matter

atom

smallest unit into which matter can be divided without the release of electrically charged particles.

element

any substance that cannot be decomposed into simpler substances by ordinary chemical processes.

molecule

a group of two or more atoms that form the smallest identifiable unit into which a pure substance can be divided and still retain the composition

pure substance

atoms & compounds(not mixtures) have a constant and definite composition

mixture

two or more substances that are not chemically combined

homogeneous mixture

a mixture where the substances are evenly distributed within the mixture

heterogeneous mixture

a mixture where the substances are not evenly distrubuted within the mixture

physical change

phase change- does not change the chemical identity of a substance.

chemical change

changes the chemical identity of a substance

oxide

a binary compound of oxygen with another element or group.

metal oxides

crystalline solids that contain a metal cation and an oxide anion.

acid

elements that donate an electron turn into these, often taste sour, conduct electricity when dissolved. 1-7 on pH scale

base

elements that accept an electron turns into these, often taste bitter, slippery to the toutch. 8-14 on pH scale

base

metal oxides in water form a(n) _____

acid

nonmetal oxides in water form a(n) ______

nonmetal oxide

a nonmetal bonded to an oxygen atom

John Dalton

reintroduced atomic theory into chemistry

plumb pudding model

model of an atom that is positively charged exept for negatively charged particles inside

Eugen Goldstein

discovered the proton

JJ Thomson

discovered the electron

cathode ray experiment

expiriment by JJ Thomson using cathode ray tubes to discover electrons

Robert Millikan

this person succeeded in precisely determining the magnitude of the electron's charge

Oil Drop experiment

experiment by Robert Milikan that measured charge of the electron

Ernest Rutherford

proposed that the negatively charged electrons surround the nucleus of an atom(planetary model)

Gold-foil experiment

Experiment by Ernest Rutherford that showed that atoms had a nucleus where most of its mass was stored

planetary model

model of an atom that show the nucleus with electrons orbiting the center on ellipse shaped paths

Chadwick

discovered the neutron

Bohr model

model of an atom with subshells surrounding the nucleus.

energy levels

on a bohr model, there are different rings, called __________ that electrons exist on.

no

can electrons exist between energy levels?

by which is closer to the average atomic mass

how can you tell which isotope is more abundant in nature?

boron-11

is boron-10 or boron-11 more abundant in nature

amu=10.81

because it is an average that includes isotopes

why is the atomic masses listed on the periodic table not whole numbers

1

mass in amu’s of proton

1

mass in amu’s of neutrons

0

mass in amu’s of electrons

1+

charge of a proton

0

charge of a neutron

1-

charge of an electron

period

a row on a periodic table, arranged in ascending order of atomic number

electron shells

each row has the same number of ___________

family

vertical groups that have a similar number of valence electrons that in turn create similar characteristics

1

How many atoms of oxygen is in H2O

4

How many atoms of oxygen is in H2SO4

36

How many atoms of oxygen is in 6 Molecules of C6H12O6

6

How many atoms of oxygen is in Fe3(CO2)3

12

How many atoms of oxygen is in Al2(SO2)6

diatomic

made up of two of the same elements

H, N, O, F, C, B, I

what elements are diatomic in nature? (there are 7, use their symbols)

ion

a variant of an element differing in charge

number of electrons

how does an ion differ from a normal atom of that element

isotopes

variant of an element differing in mass

alkali metals

high conductivity, luster, ductile, low electronegativity, low ionization

alkaline earth metals

low electronegativity, highly reactive, low ionization energy.

transition metals

good conductors, malleable, dense, high melting point

halogens

toxic, highly reactive, highly electronegative, easily form salts with metals, acidic with hydrogen

noble gases

odorless, colorless, nonflammable, low reactivity

3+

Charge of Aluminum(Al)

2+

Charge of zinc(Zn)

1+

Charge of silver(Ag)

s block

block containing alkali metals and alkali earth metals

p block

block containing nonmetals, halogens, and noble gases.

d block

block containing transition metals

f block

block containing actinides and lanthides.

metals

Characterized by having luster, malleable, ductule, and conduct heat and electricity well

nonmetals

Characterized by being dull, brittle, and poor conductors

valence electrons

electrons on the outer group

to gain stability by getting a full outer shell

why do main group elements(Groups 1A to 8A) form ions?

positive

Are metals positive or negative when they form ions

negative

are nonmetasl positive or negative when they form ions

anions

are cations or anions larger?

It moves to an inner shell

On the bohr model, what happens to an electron when energy is released?(Moves to an inner or outer shell?)

moves to an outer shell

On the bohr model, what happens to an electron when energy is absorbed?(Moves to an inner or outer shell?)

raging martians invaded venus using x-ray Guns

Phrase to remember electromagnetic spectrum from lowest to highest energy

2

Maximum number of electrons the s subshell/sublevel can hold?

6

Maximum number of electrons the p subshell/sublevel can hold?

10

Maximum number of electrons the d subshell/sublevel can hold?

14

Maximum number of electrons the f subshell/sublevel can hold?

2

How many orbitals(electron pairs) does the s subshell/sublevel have?

3

How many orbitals(electron pairs) does the b subshell/sublevel have?

5

How many orbitals(electron pairs) does the d subshell/sublevel have?

7

How many orbitals(electron pairs) does the f subshell/sublevel have?

Potassium Bromide

Name of this formula: KBr

Ionic

Is potassium Bromide(KBr) ionic or covalent compound

Calcium diflouride

Compound name for this formula: CaF2

covalent

Is calcium diflouride(CaF2) ionic or covalent

CCl4

Coumpound formula for Carbon tetrachloride

covalent

Is carbon tetrachloride(CCl4) ionic or covalent

nitrogen trihydride

Compound name for this formula: NH3

covalent

is nitrogen trihydride(NH3) ionic or covalent

ide

When naming covalent compounds what suffix do you add to the last nonmetal

mono di tri tetra penta hexa hepta octa nona deca

When naming covalent compounds what prefixes do you use to indicate the number of that atom or relement

true

true or false, if the first element has only one of that element, instead of writing mono, you just use the element name

carbon monoxide

name this covalent compound:

CO