Chemistry (Grade 10)

Matter

Anything that has mass and takes up space, classified through particle

Particle Theory

• All matter is made up of tiny particles

• All particles in a pure substance are the same

• Particles attract each other

• Particles are in constant motion

• higher temperature cause particles to move faster

Classification of Matter

A pure substance or mixture

pure substance

one type of particle - ex: Distilled water (compound) or Oxygen (Element)

they have different properties because they are composed of different particles

Element

A pure substance that cannot be broken down further (not physically or chemically)

• found on periodic table

• ex: Helium, Calcium, Gold

Compound

Pure substance that are made of 2 or more different elements that are chemically combined

• Can be broken down by chemical methods

Mixture

More than one type of particle in a substance

ex: air - mostly nitrogen

Solution

• Cannot see all different particles, blended to look like one

• Also known as (aq) can be dissolved in water

Mechanical mixture

All components are visible - Ex: pizza

Properties of matter

described with physical or chemical properties for elements + Compounds

physical property

Characteristic of a substance that can be observed/measured without changing its identity

qualitative properties

Characteristics determined by senses

ex: state, colour, odour, lustre, texture and malleability

chemical property

Characteristic behaviour when a new substance is formed

The ability for a substance to react with another substance and form one/multiple substances

ex: combustibility, reaction with oxygen/acid/substances, decomposition (substance breaks down into parts it made up of)

quantitative properties

measurable characteristic

ex: viscosity (less viscous - easy to pour), melting point, boiling point, solubility, hardness (to scratch another material), conductivity and density

physical change

The substance has changed state/form with new properties, but no new substance is created and it is reversible, as well as particles remain the same. !DISSOLVING!

Chemical change

Always causes at least one new substance, usually impossible to reverse (unless you are a rechargeable battery or light bulb).

Clues: new odour/colour, heat or light given off (energy), bubbles, precipitate ( 2 L → 1 S), difficult to reverse

number of elements are in a pure substance

1 or more, depending is the pure substance is made up of 1 element or a compound with multiple elements.

3 subatomic particles

Protons: equal atomic number, make up mass (1), positive, do not move, in nucleus

Neutrons: are the mass subtracted by the protons, make up mass (1), neutral, do not move and in nucleus

Electrons: no mass, negative, equal # of protons if neutral, orbit the nucleus

metals and their properties

They are the first two families, shiny, malleable, solid (except mercury at room temp). React to water

Nobel Gases

Nobel gases are elements found in the last row of the periodic table, they are fairly inert (unreactive) due to having a full valence shell and not require electrons to be stable

Non-metals

they are the last 6 groups on the periodic table, which are dull, liquid, gas, brittle solid

Metalloids

Have properties of metals and non-metals, on staircase

Halogens

2nd last column, poisonous and react with metals

Most reactive elements

Francium (metal) and Fluorine (non-metal)

Bohr-rutherford diagram

• Electrons farther from the nucleus have more energy (to leave) then ones closers

• small circle with # of p + n in middle and then electrons outside that shell

• 12, 6, 9, 3

• electrons occupy specific energy levels (shells/orbits)

Properties of elements

Are determined by the arrangement of the electrons in the outmost occupied energy level (valence)

• valence also determine how a atom will react

• atoms in the same families = same valence = react similarly

Atoms bonding

a chemical reaction where they sharing, losing or gaining electrons

Full outer shell

provides chemical stability

Isoelectric

When a atom has the same particle arrangement as nobel gas. (same valence amount)

• atoms are most stable when isoelectric

• the closer an atom is to be isoelectric the more reactive it is

Reactivity trend for metals

they lose electrons easier, they become more reactive as you go left (decrease in atomic number) and as you go down (more shells) Creates cations (positively charged ions)

Reactivity trend for non-metals

Gain electrons, more reactive with less shells (up) and as you go right (more electrons) because it makes it easier to gain a few electrons and become stable. Creates anions (negatively charged ions)

Ions

charged atoms or molecules that have either gained or lost electrons

ionic bond

two ions held together by a strong electrostatic force of attraction

Purpose of Ions

to become stable, atoms will gain/lose electrons to have a full outer shell, they will also become isoelectric

Nomenclature

Does the bond have a metal

Yes:

• metal + non metal(ide) = binary

  Does the metal have different valence amounts?

  Yes:

  • Transition metal (roman numeral) + non metal(ide) = multivalent

  Is the non metal actually a group of atoms that tend to stay together with a overall ionic charge (2+ nonmetals)?

  Yes:

  • Transition (RN) /metal + polyatomic = polyatomic

No:

• its molecular

• uses prefixs to tell # of atoms

• mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

• never use mono on the first element

• can not be reduced

Diatomic Molecules

Have No Fear Of Ice Cold Beer

Hydrogen

Nitrogen

Fluorine

Oxygen

Iodine

Chlorine

Bromine

molecular compound

involves a non-metal bonding covalently to another nonmetal

they share valence to become stable

Covalent

Electrons are shared between atoms, electrons are attracted to the nucleus of both atoms

S, L, G, Aq

S = Solid

L = Liquid

G = Gas

Aq = Aqueous - Dissolve in liquid

Rules of Word Equations and Skeleton

• The skeleton equation requires the symbols WITH the state and arrow to show products

• words are simple

form: Reactant(s) → Product(s)

Law of conservation of Mass

Mass of reactants must equal mass of products, same number of atoms in both reactants and product side WITHOUT CHANGING FORMULA

tips:

• increase atoms ONLY

• balance elements last

• balance compounds then metals first

• only works if formula is correct

• if polyatomic stays together in reactants and products, they can stay as one

• KEEP STATES LABELED

Synthesis Reaction

When two reactants join together to produce one product (A large compound)

Decomposition Reaction

When a large compound break down into two or more separate products

Single Displacement

When one element is displacing another in a compound

AC + B → A +BC

or AC + B → C + AB

Double Displacement

Involves one component of both molecules(compounds) being exchanged

AB + CD = AD + CB

Combustion

When a substance reacts/joins with oxygen

ex: Mg + O

Hydrocarbons - when hydrogen and carbon are reacting with oxygen, they can produce water and carbon dioxide. If there is insufficient amount of oxygen, it can create: water, carbon dioxide, carbon monoxide, and solide carbon

Acid Properties

• Produces H+ ions

• corrosive

• sour

• reacts with electricity

• some are edible

• cause severe burns

Base Properties

• Produces OH- ions

• Bitter

• Corrosive

• reacts with electricity

• some are edible

• SLIPPERY

• cause severe burns

How to write an acid

• binary: Hydro(non-metal root)ic acid

  • H depends on charge of non metal

• Oxyacids - Polyatomics must have oxygen in it

  • Ends with ate (polyatomic)ic acid

  • Ends with ite (polyatomic)ous acid

What is a base

compound including (polyatomic - OH), that produces OH- (aq) ions when dissolved in water (called dissocation)

Bases were discovered from soap, the first base to be created

• some safe to eat like baking soda but some deadly

• remedies like antacids ( weak base)

What is a acid?

It is a compound that produces Hydrogen ions H+ (aq) when dissolved in water (called ionization)

Ex: vinegar in your home, soda, candy or citrus fruit

Why can aqueous bases and acids conduct electrical current?

because of the charged ions that are made when dissolving water

• ions separate from one another

ph Levels

7 and lower is acids - the lower the number the more acidity the acid has - more h then OH

7 and higher is bases - the larger the number the more strong it is - more OH then H

7 is neutral, like water or blood

Indicators

• Help tell the difference between bases and acids

• compounds change colour to changes in concentration of Hydrogen Ions or hydroxide ions

• for example, the filter paper turning pink was a indication of a base

• litmus red paper - red = acid / blue = base

• litmus blue paper - red/pink = acid / blue = base

What are the hydrogen atoms in a acid responsible for?

The acidic properties

What is water?

It is HOH, which makes it neutral and breaks down into charged atoms (H) and (OH)

How to avoid teeth erosion

Avoid acidic foods like soda, and citrus fruit

tart = sour

NH4 AND NH3, CH4

Ammonium and ammonia, methane