Chemistry midterm review

Boyle’s law

pressure increases volume decreases

temperature constant

more collisions in smaller space so more pressure

Boyle’s law formula

p1v1=p2v2

Charles law

volume increases as temperature increases

pressure is constant

Charles’ law formula

V1/T1=V2/T2

Gay Lussac’s law

pressure increases as temperature increase

volume remains constant

Gay Lussac’s law formula

p1/t1=p2/t2

Combined gas law

No constant needed

P1V1/T1 = P2V2/T2

where is the atomic number

the bottom number

what does the atomic number show

the number of protons

where is the mass number

the top number

what does the mass number show

mass of protons and neutrons

how to find the number of electrons in a neutral atom

its equal to the number of protons

isotopes protons and neutrons are…

the same number of protons but different numbers of neutrons

what is this?

watchglass

what is this?

burette

what is this?

graduated cylinder

what is this?

beaker

what is this?

erlenmeyer flask

what is this?

volumetric flask

Fusion

Combining two or more smaller nuclei into one larger nucleus 

Mass stays constant through the reaction (rxn)

Fission

One large nucleus splits apart into two or more smaller nuclei

Chain reaction started by firing a neutron at a nucleus

half life

Time for HALF of a radioactive substance to decay

#of half lives = time passed/half life

Orbitals

aka electron cloud

where electrons most likely are

S-orbitals

sphere shape

left chunk on periodic table

starts 1s

P-orbitals

propellor shape

right chunk on periodic table

starts 2p

D-orbitals

Daisy shaped

middle chunk on periodic table

starts 3d

F-orbitals

flower shaped

bottom chunk on periodic table

starts 4f

Energy Level

Size of the orbital

Electron configuration

this format

1s² 2s² 2p⁶

Aufbau principle

Ausbau says Always lowest first 

fill the lowest first

Hund’s rule

Hund says they hate each other

Separate into different rooms until they have to double up 

Pauli exclusion principle

Pauli’s prefer to face opposite

electrons in an orbital spin opposite directions

isoelectronic

atoms with same number of electrons

+or - to make the same

When losing electrons take from largest number

 λ

wavelength

• length of one complete wave cycle

• m, nm, etc.

ν

frequency

Amount of waves that pass a point during a period of time

Hz

E

energy

joules

E = hc/ λ

finds energy using Planck’s constant, speed of light, and wavelength

E = hν

finds energy using Planck’s constant and frequency

c= λν

finds speed of light using wavelength and frequency

highest energy to lowest

highest

• gamma rays

• violet

lowest

• radio waves

• red

longest wavelength to shortest

longest

• radio waves

• red

shortest

• gamma rays

• violet

metals

middle and left side of periodic table

Likes to lose electrons (losers)

nonmetals

right side of periodic table

Like to gain electrons

Based on electronegativity

where are metalloids on the periodic table

in a “staircase” between metals and nonmetals on right side

main group elements

the s and p groups

transition metals

the d (middle) group

inner transition metals

f group (bottom)

atomic radius

the size of atom

adding protons pulls electrons closer to nucleus so radius shrinks

Increases to the LEFT and DOWN

ionic radius

an elements share of the distance between adjacent ions in an ionic solid

Comparing an atom of an element to the ion it forms

Electron Affinity

amount of energy needed or given off when neutral atom gains electron

Electronegativity

how likely atom is to gain electron from another atom

• Wants to be stable so steals from other atoms

Smaller atom = higher electronegativity

Ionization

IE

Energy needed to remove electron from atom

Increases UP and to the RIGHT the periodic table

opposite of atomic radius bc in small atoms electrons are close to nucleus where attraction on stronger

chemical reactivity

How likely/much an element reacts with another substance

how easily electrons can be removed (ionization E)

how attracted they are to other atom’s electrons (electronegativity).

Nonpolar covalent bond

• Electron shared equally 

  • Electronegativity  difference is 0.0-0.3

• Usually identical atoms

Polar covalent bond

• Electrons shared unequally

  • Electronegativity difference is 0.3-1.7

• Results in partial charges - dipole

  • More electronegative side has particle negative charge