Comprehensive Chemistry Review: Matter, Atomic Structure, Bonding, and States of Matter

Matter

Anything that has mass and takes up space.

Element

A single type of atom.

Compound

Two or more elements chemically bonded.

Mixture

Two or more substances mixed, variable composition.

Particle Theory

A theory that explains the properties of matter in terms of particles.

States of Matter

The distinct forms that different phases of matter take on.

Pure Substance

One kind of particle, fixed composition.

Homogeneous Mixture

Uniform composition, looks the same throughout.

Heterogeneous Mixture

Not uniform, parts visible.

Periodic Table

A table that organizes elements by increasing atomic number and groups.

Physical Properties

Characteristics that can be observed without changing the substance.

Chemical Properties

Characteristics that describe how a substance interacts with other substances.

Atomic Structure

The arrangement of protons, neutrons, and electrons in an atom.

Bohr-Rutherford Diagram

A diagram that shows the arrangement of electrons in an atom.

Lewis Dot Diagram

A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons.

Ionic Bonding

The electrostatic attraction between oppositely charged ions.

Molecular Bonding

The sharing of electrons between atoms.

Density Formula

Density = mass/volume.

Temperature and Particle Motion

Higher temperature means faster particle motion.

Cooling Metal

Cooling lowers particle kinetic energy, causing particles to vibrate less and move closer.

Metals

Elements that are typically shiny, malleable, ductile, and good conductors.

Non-Metals

Elements that are typically dull, brittle, and poor conductors of heat and electricity.

Metalloids

Elements that have properties intermediate between metals and non-metals.

Metal reactivity trend

Metal reactivity decreases from left to right.

Non-metal reactivity trend

Non-metal reactivity increases from left to right.

Metal reactivity trend (vertical)

Metal reactivity increases from top to bottom.

Non-metal reactivity trend (vertical)

Non-metal reactivity decreases from top to bottom.

Li vs Be reactivity

Li is more reactive than Be.

F vs O reactivity

F is more reactive than O.

Na vs Mg reactivity

Na is more reactive than Mg.

Cl vs S reactivity

Cl is more reactive than S.

Alkali Metals

Elements: Li, Na, K, Rb, Cs, Fr. Properties: one valence electron, very reactive, soft, conductors. Location: Group 1, leftmost column.

Alkaline Earth Metals

Elements: Be, Mg, Ca, Sr, Ba, Ra. Properties: two valence electrons, reactive but less than alkali, harder than alkali. Location: Group 2, second column.

Halogens

Elements: F, Cl, Br, I, At. Properties: seven valence electrons, very reactive non-metals, form salts with metals. Location: Group 17, right side.

Noble Gases

Elements: He, Ne, Ar, Kr, Xe, Rn. Properties: full valence shell, very low reactivity, gases at room temp. Location: Group 18, far right column.

Copper wire properties

Shiny, good conductor.

Glass of milk properties

Cloudy, opaque.

Candle properties

Solid at room temp, melts when heated.

Aluminum foil properties

Thin, malleable.

String lights properties

Flexible wires, conduct electricity.

Spoonful of sugar properties

Crystalline, dissolves in water.

Physical change example

Tailor makes a suit from fabric — physical change, no new substance.

Chemical change example

Logs burnt in a campfire — chemical change, new substances form (ash, smoke).

Substance color change

Substance changes colour in acid — likely chemical change, indicates a new chemical state.

Physical change definition

Alters form or state, no new substance.

Chemical change definition

Makes a new substance, bonds break and form.

Water freezing

The molecules stay H2O. Only particle motion and arrangement change. No new substance forms.

Metallic lustre

Physical property.

Substance explosion

A substance explodes when ignited — chemical property.

Boiling point

Physical property.

Color change in water

A substance changes colour when mixed with water — chemical property if colour change comes from a reaction.

Water boiling

Water boils to steam — physical change.

Wood sawing

Wood is sawed into a toy box — physical change.

Firewood burning

Firewood burns to ash — chemical change.

Orange crystals in water

Orange crystals stirred into water (drink mix) — physical change (dissolving).

Baking cookies

Sugar, eggs, flour mixed and baked into cookies — chemical change, new substances form.

Bohr-Rutherford model

Place protons in nucleus, neutrons in nucleus, electrons in shells (first shell 2, second shell 8, third shell 8 for these examples).

Lewis dot structure

Lewis dots show only valence electrons around the symbol.

Lithium (Li) details

Protons 3, neutrons 4, electrons 3. Shells: 2,1. Lewis: one dot.

Carbon (C) details

Protons 6, neutrons 6, electrons 6. Shells: 2,4. Lewis: four dots.

Neon (Ne) details

Protons 10, neutrons 10, electrons 10. Shells: 2,8. Lewis: eight dots.

Hydrogen

H (Z=1, mass≈1). Protons 1, neutrons 0, electrons 1. Shells: 1. Lewis: one dot.

Chlorine

Cl (Z=17, mass≈35). Protons 17, neutrons 18, electrons 17. Shells: 2,8,7. Lewis: seven dots.

Magnesium

Mg (Z=12, mass≈24). Protons 12, neutrons 12, electrons 12. Shells: 2,8,2. Lewis: two dots.

Argon

Ar (Z=18, mass≈40). Protons 18, neutrons 22, electrons 18. Shells: 2,8,8. Lewis: eight dots.

Silicon

Si (Z=14, mass≈28). Protons 14, neutrons 14, electrons 14. Shells: 2,8,4. Lewis: four dots.

AlBr3

Al 1, Br 3. Total atoms 4.

FeF2

Fe 1, F 2. Total atoms 3.

Na3P

Na 3, P 1. Total atoms 4.

LiNO3

Li 1, N 1, O 3. Total atoms 5.

AgNO3

Ag 1, N 1, O 3. Total atoms 5.

Si(OH)4

Si 1, O 4, H 4. Total atoms 9.

3 NaCN

Na 3, C 3, N 3. Total atoms 9.

2 Ca(NO3)2

Ca 2, N 4, O 12. Total atoms 18.

Na3PO4

Na 3, P 1, O 4. Total atoms 8.

4 PBr3

P 4, Br 12. Total atoms 16.

Atomic number

Number of protons.

Electrons

Equal to protons for neutral atoms.

Neutrons

≈ rounded atomic mass − atomic number.

Ionic compounds

Form between metals and non-metals.

Molecular compounds

Form between non-metals.

Ionic transfer

Electrons, forming ions.

Molecular share

Electrons, forming covalent bonds.

Density

Mass / volume.

Given mass 2800 g, volume 3 cm3

Density = 2800 ÷ 3 = 933.3 g/cm3.

Mass 1200 kg, volume 2.0 m3

Density = 1200 ÷ 2.0 = 600 kg/m3.