chem grade 10

Matter

Anything with volume and mass; made up of tiny particles.

Energy

Ability to do work (heat, light, sound, electricity).

Matter vs Energy

Matter is studied in chemistry; energy in physics.

Pure Substances

Made of one type of particle; can be elements or compounds.

Mixtures

Contain two or more substances; can be homogeneous (uniform) or heterogeneous (non-uniform).

Particle Theory

All matter is made of tiny particles.

Physical Properties

Color, smell, size, volume, density, texture, mass.

Chemical Properties

Flammability, reactivity, rusting, corrosiveness, burning, acidity.

Physical Change

Change in form or state; no new substance formed; reversible.

Chemical Change

New substance formed; often irreversible; signs include new odor, color, or gas.

Hardness

Resistance to damage.

Ductility

Ability to be stretched into wire.

Clarity

Degree to which a substance is transparent.

Malleability

Ability to be hammered into sheets.

Solubility

Ability to dissolve in another substance.

Boiling (Evaporation)

Liquid changing to gas.

State

Whether substance is solid, liquid, or gas.

Lustre

How shiny a substance is.

Density

Ratio of mass to volume.

Proton (p)

Positive charge, relative mass 1, in nucleus.

Neutron (n)

No charge, relative mass 1, in nucleus.

Electron (e)

Negative charge, relative mass 1/2000, in shells.

Electron Shells

First shell holds 2 electrons, then 8, then 8.

Bohr-Rutherford Diagram

Model showing electron arrangement around nucleus (useful for first 20 elements).

Valence Electrons

Electrons in outer shell; determine reactivity and bonding.

Groups (Columns)

18 vertical groups.

Periods (Rows)

7 horizontal periods.

Group 1

Alkali Metals.

Group 2

Alkaline Earth Metals.

Groups 3-12

Transition Metals.

Group 14

Metalloids.

Group 17

Halogens.

Group 18

Noble Gases.

Ionic Bonding

Transfer of electrons from one atom to another.

Metal (Cation)

Tends to lose electrons (left side of table).

Non-Metal (Anion)

Tends to gain electrons (right side of table).

Stability Rule

Metals lose to empty outer shell; non-metals gain to fill shell.

Example

Na⁺ + Cl⁻ → NaCl (sodium chloride).

Binary Ionic Compound

Compound composed of two elements (metal + non-metal).

Monovalent Element

Has only one possible ion charge.

Naming Rule

Write cation (metal) name first.

Multivalent Elements

Elements with more than one possible ion charge.

Polyatomic Ions

Ions made of more than one atom acting as a single charged particle.

Properties

Stay together during reactions; not binary; usually contain non-metals.

Naming

Write cation first, then polyatomic ion (no ending change).

Formula Writing

Identify each ion and its charge.

Common Polyatomic Ions

Ammonium (NH₄⁺)

Covalent Bond

Sharing of electrons between atoms.

Molecular Compound

Formed when atoms share electrons through covalent bonds.

Metallic Bond

Found in metals/alloys; electrons are free to move ('sea of electrons').

Alloy

Mixture of two or more elements, with at least one metal.

Lewis Dot Diagrams

Model showing only valence electrons of an atom.

Stable

When outer shell full (8 electrons; 2 for H & He).

Positive ions

Cations.

Negative ions

Anions.

Ionic Bond

Transfer of electrons between a metal and a non-metal.

Chemistry

The study of matter, its properties and its changes or transformations.

Mixture

The combination of 2 or more different substances that mix very well or don't.

Homogenous

2 or more different substances that mix very well, hard to separate, transparent except alloys (Eg. salt water, sugar water, glass).

Heterogenous

2 or more different substances that don't mix very well (Eg. Pizza with toppings, salad, raisin cookie).

Compounds

Pure substances that contain 2 or more elements with a fixed composition, including a chemical formula.

Elements

Pure substances that cannot be broken down into smaller parts, found on the periodic table.

Solid

Atoms tightly condensed, mainly hard and strong.

Liquid

Atoms loosely condensed, mainly flowy.

Gas

Atoms not condensed, can flow through air.

Combustibility

ability of a substance to burn in air, producing heat and light

Decomposition

change that can occur when a substance is broken down into the parts that make it up

Reactivity with Oxygen

change that can occur when a substance is exposed to oxygen

Reactivity with Acids

change that can occur when a substance is exposed to acid

Reactivity with Other Substances

change that can occur when one substance reacts with another substance.

Qualitative

something that can't be measured, based on physical quality

Quantitative

something that can be measured and has a numerical value

Chemical Changes

Substance changes into another substance, chemical formula is different, can't be undone easily, precipitate can be created.

5 Clues to Find Chemical Change

A new color appears, Heat or light is given off or absorbed, Bubbles of gas are formed, The change is difficult to reverse, Precipitate is formed

Hydrogen (flaming splint)

put flaming splint and hydrogen next to each other, squeaky noise will be made because hydrogen is explosive.

Oxygen (glowing splint test)

put glowing splint in oxygen, splint will ignite because oxygen supports combustion.

Carbon Dioxide (burning splint, limewater)

burning splint extinguishes near carbon. Lime water (clear) and carbon dioxide mixed creates a white creamy precipitate.

Water Vapour (Cobalt (II) Chloride paper)

Cobalt (II) Chloride paper (blue) near water vapour becomes pink.

Alkali Metals

Group # 1, Valence Electrons: 1, Physical Properties: Solids, Shiny, silvery color, Soft metals, Chemical Properties: Extremely reactive, React with water to produce hydrogen gas, Found in nature only as compounds, Lose 1 electron form +1 ions

Alkaline Earth Metals

Group # 2, Valence Electrons: 2, Physical Properties: Solids, Metals, Denser than group 1, Chemical Properties: Very reactive, Found in nature only as compounds, Lose 2 electrons form +2 ions

Halogens

Group # 7, Valence Electrons: 7, Physical Properties: Nonmetals, Multi colored, Astatine - radioactive, Chemical Properties: Extremely reactive, Very corrosive, Found in nature only as compounds, Gains 1 electron to form -1 ions

Noble Gasses

Group # 8, Valence Electrons: 8, Physical Properties: Nonmetals, Gasses at room temperature, Odourless, colorless, tasteless, Stable electron structure, Chemical Properties: Very stable, Unreactive because of full outer shell electrons, Almost never combine with other elements, Do not gain/lose electrons

Transition Metals

Location: In between groups 2-13 (including elements below the main section), Properties: They are good conductors of heat and electricity, They are malleable, They have high melting points, They are hard/tough, They have high densities.

Standard Atomic Notation

The way a chemical element is written. Mass at the top left corner, atomic number at the bottom left corner, and the element in the middle. Always round numbers.

Bohr Rutherford Diagram

The way an atom is drawn, named after the scientists Ernest Rutherford and Niels Bohr. These diagrams include the shells of the atom, a labeled nucleus with a written number of protons and neutrons, an element symbol, and electrons drawn on each shell.

Louis Dot Diagrams

The way an atom is drawn but with only the valence shell (outermost shell). The element symbol is in the middle and the electrons are placed around it as if there was a shell drawn there.

Electron

Negative charge (in orbit)

Proton

Positive charge (in nucleus)

Neutron

No charge (in nucleus)

Ion

The charge an atom has, either positive, negative or neutral.

Cation

An atom with a positive charge.

Anion

An atom with a negative charge.

Unstable Atom

An atom with a valence shell that is not complete.

Stable Atom

An atom with a valence shell that is complete.

Periodic Table

An organized arrangement of chemical elements into rows (Periods) and columns (groups).

Ionic Compound

Metal + Non Metal.

Covalent Compound

Non Metal + Non Metal.

Monovalent

Only 1 possible Valence.

Multivalent

Multiple possible Valences.

Binary

2 different elements.