MYP Chemistry Final Review

ionic

non-metal and a metal

covalent

non-metal and a non-metal

synthesis

two elements react to form one product

single replacement

one element and one compound react and switch partners

double replacement

two compounds switch partners

decomposition

one compound breaks into pieces

combustion

compound or element reacts with 02

atomic number

stands for the number of protons

mass number

mass of the nucleus, protons and neutrons

ion

charged element

isotope

element with same number of protons, but different number of neutrons

average atomic mass

weighted average of all known isotopes of an element

J.J. Thomson

-Cathode Ray Tube

-discovered electrons

-evenly distributed in a + sphere

Ernes Rutherford

-Gold Foil

-atoms are mostly empty space

-atoms have a positively charged nucleus

-electrons moved around nucleus at a distance

How did Bohr contribute to Rutherford's atomic model?

-electrons can only exist on definite energy levels

How are elements in the same group related?

They have the same number of energy levels

How are the alkali metals all related?

They all have a +1 charge

How are all the noble gases related?

They all have 8 electrons

As wavelength gets shorter, frequency...

increases

As wavelength gets shorter, energy...

increases

What is the electromagnetic spectrum? What is the highest energy wave? Lowest?

The entire spectrum/continuum of energy

-lowest: radio

-highest: gamma ray

What is the difference between a bright line spectrum and a continuous spectrum?

The continuous spectrum is ALL visible & the bright line spectrum is when certain/discrete light waves are present

Explain how electron movement between energy levels produces photons of light.

When electrons move down energy levels, energy is released. When they move up energy levels, energy is absorbed instead.

How do waves of red light and blue light differ with frequency, wavelength, and energy?

Red light has a lower frequency and energy, and a longer wavelength

Electronegativity

attraction for additional electrons

Ionization energy

amount of energy required to remove an electron

Atomic radius

the radius of an atom

What are some distinctive properties of ionic compounds?

Ionic compounds have a metal & non-metal attracted to each other due to the electrostatic attractions.

What makes an ionic bond different than a covalent bond?

An ionic bond does NOT have two non-metals and is stronger than a covalent bond.

What is VSEPR theory?

When there may be lone pairs or even shared/bonded pairs, putting the atoms together

dipole-dipole

polar covalent bonds

london dispersion forces

non-polar covalent bonds

hydrogen bonds

must have hydrogen AND N, O, or F

What are some properties of the types of bounds?

Ionic bonds are created due to the transfer of electrons.

Covalent bonds are created due to the sharing of electrons.

Network bonds are multiple atoms all interconnected by attraction.

Solid

-rigid, locked

-little free space

-high pressure

Liquid

-move/slide past

-little free space

Gas

-move past one another

-lots of free space

-low pressure

matter

anything that has mass and takes up space

pure substance

made up of only one element or compound

homogeneous mixture

when like substances are blended together

heterogeneous mixture

when different substances are blended together

element

most basic component of all matter

atom

is what matter is made up of

compound

chemically combined element

What are the two types of mixtures?

homogeneous and heterogeneous

Give three examples of physical properties

color, shape, luster, density

Give three examples of chemical properties

color change, bubbles form, precipitate forms, heat formed

solute

substance added to the solution, is dissolved

solvent

substance doing the dissolving

solution

the solute and solvent together

concentration

the amount of solute in an amount of solvent

electron configuration

S, D, P, F

1 mole

22.4 L

atoms, ions, molecules, or formula units

6.02 X 10 ^23

concentration is measured by

M = mole/liters

dilution is measured by

M1V1 = M2V2

law of conservation of mass

initial concentration & volume = final concentration & volume in a dilute

proton mass

1 amu

neutron mass

1 amu

electron mass

1/1840 amu

ground state electron

when electrons are placed by the periodic table order

excited state electron

when 1 electron has been "promoted" to a new energy level & location

Nitrite

NO2

Nitrate

NO3

Sulfate

SO4

hydroxide

OH

phosphate

PO4

carbonate

CO3