Chemistry Review 1

Properties of Matter

100

The 2 properties of Matter

Chemical properties and Physical Properties

200

Solid, Liquid, Gas, and Plasma Are

States of Matter

300

Definite shape and volume

Solid

400

Properties like color, density, melting/boiling point etc

Physical properties

500

Depend on the amount of matter (e.g. mass, volume)

Extensive Properties

Structure of Atom

100

The 3 subatomic particles

Protons, electrons, and neutrons.

200

The charges and location of the subatomic particles

• Protons: Positively charged particles found in the nucleus.
• Neutrons: Neutral particles also in the nucleus.
• Electrons: Negatively charged particles in orbitals around the nucleus.

300

Mass Number Formula

Mass Number= Protons+ Neutrons

400

The number of protons in an atoms nucleus it defines the element

Atomic Number

500

Atoms of the same element with different numbers of neutrons

Isotopes

Electron Configuration

100

Each energy level contains sub-levels known as orbitals

s, p, d, f

200

The first energy level holds 2 electrons, the second holds

8

300

Can hold up to 10 electrons

d-orbital: Can hold up to 10 electrons.

400

Maximum number of electrons the 2nd electron shell can hold

the second holds 8

500

 1s² 2s² 2p⁶ 3s² 3p⁶ 3d³ 4s²

Vanadium V

Periodic Table

100

Vertical columns in the periodic table. Elements in the same group have similar chemical properties.

Groups: Vertical columns in the periodic table. Elements in the same group have similar chemical properties.

200

Horizontal rows in the periodic table. Properties change gradually across a period.

Periods: Horizontal rows in the periodic table. Properties change gradually across a period.

300

How many groups and rows do the periodic table have

18 groups

7 rows

400

The element Sb metal, metalloid, nonmetal. Atomic number 

Metalloid, 51

500

F block contains

Lanthanide and Actinide

Periodic Trends

100

The distance from the nucleus to the outermost electron shell

Atomic Radius

200

Atomic Radius trend: left to right

Decreases across a period (left to right) due to increased attraction between protons and electrons.

300

Ionization Energy trend: left to right

Increases across a period (left to right) because it becomes harder to remove an electron as the number of protons increases.

400

Electronegativity trend: top to bottom/ down

Decreases down a group due to the increasing distance of the outer electrons from the nucleus.

500

Become more reactive as you move down a group. 

Metals, Metalloids, Non-metals

Metals: Become more reactive as you move down a group.

 Non-metals: Become more reactive as you move up a group.