SNC1W Chemistry Review

Vocabulary practice flashcards covering particle theory, classification of matter, physical and chemical changes, periodic table families, atomic theories, and ions/molecules from the SNC 1W Chemistry Review.

Particle Theory of Matter 5 main ideas

1. All matter is made of tiny particles; 2. Particles are always moving; 3. There is always space between all particles; 4. Adding heat makes particles move faster; 5. All particles in the same substance are the same, while different substances are made of different particles.

Solid

particles are tightly packed together and molecules move freely, having a definite volume and taking the shape of the container.

Liquid

particles are less tightly packed and molecules move quickly and freely, definite volume and taking the shape of the container.

Gas

particles are widely spread apart and move quickly and freely; it has no fixed volume or shape, expands to fill the container it is placed in, and takes shape and volume of the container.

Melting

A change of state from solid to liquid caused by adding heat (example: an ice cube melting in the sun).

Freezing

A change of state from liquid to solid caused by removing heat (example: water turning into ice in a freezer).

Evaporation

liquid to gas caused by adding heat (example: wet clothes drying in the sun).

Condensation

gas to liquid caused by removing heat (example: water droplets forming outside of a cold glass).

Sublimation

solid to gas caused by adding heat (example: dry ice changing to a gas without becoming a liquid).

Deposition

gas to solid caused by removing heat (example: frost forming on a cold window).

Pure Substances

made up of atoms on the periodic table and cannot be physically separated.

Element

A pure substance made of the same type of atoms found on the periodic table (examples: Na, O, Ca).

Compound

A pure substance that has 2 or more different atoms attached (bonded). Periodic table Ex H2O

Mixture

substances are made from many pure substances and can be separated.

Homogeneous Mixture (Solution Mixture)

A mixture that is uniform, looks the same, and substances mix well together (example: apple juice).

Heterogeneous Mixture (Mechanical Mixture)

A non-uniform mixture where different parts can be seen because the substances do not mix well together (examples: granola bar, Caesar salad).

Qualitative Observation

An observation that describes qualities of matter using words.

Quantitative Observation

An observation that uses numbers or measurements.

Physical Property

appearance, what they look like (examples: lustre (shiny), clarity (transparent), viscosity(low=fast flow), hardness, state,

Chemical Property

how a substance reacts with something else. Ex combustion, flammability

Physical Change

A change in shape, size, or state in which no new substance is formed, and that is easy to reverse (example: ripping a piece of paper).

Chemical Change

produces a new substances and is difficult to reverse.

5 Clues of a Chemical Change

1. New colour; 2. New odour/smell; 3. Heat or light; 4. Bubbles of gas appear; 5. A new solid is formed.

Density

The amount of mass per unit of volume for a substance, mass in grams ($g$) volume in cubic centimeters ($cm^3$), density units of $g/cm^3$.

Group 1: Alkali Metals

known for their softness; physical properties include being soft, bright, grey, and shiny; chemical property being reactive with air.

Group 2: Alkaline Earth Metals

reactive metals found in earth materials and bones; physical properties include being shiny and silver-white; chemical property burning with colourful flames.

Groups 3-12: Transition Metals

unique for mercury being the only transition metal that becomes a liquid at room temp. Physical properties, hard, highly dense, chemically, do not catch fire easily

Group 17: Halogens

Unique for The most reactive nonmetals on the periodic table; physical properties highly toxic, existing in all three states (solid, liquid, gas), and an unpleasant smell; chemical property is being highly reactive, especially with alkali metals.

Group 18: Noble Gases

unique for known as oxygen family; physical properties colourless and odourless; chemical property includes glowing in neon signs.

Hydrogen ($H$)

Unique for The lightest element in the universe; physically a colourless and odourless gas, and chemically a highly flammable gas.

Actinides

unique for known as 'rare earth elements' physically silvery-white and dense, and chemically highly reactive.

Lanthanides

Chemicals similar to one another physically silvery-white and soft, and chemically tarnish quickly in the air.

Democritus

proposed that all matter is made of tiny particles called atoms, Greek word 'atomos' meaning uncuttable.

Aristotle

believed that matter was made of four elements: fire, earth, water, and air.

John Dalton

comparing the atom to a billiard ball.

J.J. Thomson

compared the structure of atom to a blueberry muffin or plum pudding.

Ernest Rutherford

conducted the gold foil experiment to develop atomic theory.

Niels Bohr

proposed electrons are placed in orbit around a positive centre.

James Chadwick

The scientist who discovered neutrons.

Bohr-Rutherford Model

The current model of the atom orbits electrons with the nuclear core.

Ion

An atom that has gained or lost electrons

Cation

A positively charged ion formed when an atom loses electrons; (metal) for example, a charge of $2+$ means loss of 2 electrons.

Anion

A negatively charged ion formed when an atom (non-metal) gains electrons; for example, a charge of $1-$ gain of 1 electron.

Molecular Element

Molecules having the same elements

Molecular Compound

Molecules that consist of two or more different elements

Why are alkali metals so reactive

Want to lose 1 electron since they have 1 valence electron

Why are noble gases boring

Already have a full shell, don't need to gain, lose, or share electrons

What do all elements in the same group have in commen

Same # of valence electrons by group #

What do elements in the same period have in common

Period # = # of shells needed

What holds ions together in a ionic compound?

Ionic bond

Metals

Hard solid shiny, good conductors of heat and electricity

Non metals

Soft elements poor conductors of heat and electricity

Metalloids

Share properties or metals and some non metals solid at room temp week conductors of electricity