Grade 9/10 Chemistry

Front 1

Periodic Table

Back 1

Organized chart of the elements according to increasing atomic number. A different font means it is not from Earth.

Front 2

Elements

Back 2

Substance made from one kind of atom. Dimitri Merideleu arranged these by property. A pattern can be seen when arranged by atomic number by similar patterns. It occurs in columns.

Front 3

Compound

Back 3

Substance made of two or more elements.

Front 4

Atomic Number

Back 4

Henry Mosela developed this concept. This is equal to the amount of protons in an atom, and used to identify any known element.

Front 5

Modern Atomic Theory

Back 5

The atom is composed of three subatomic particles: protons, neutrons and electrions.

Front 6

Protons

Back 6

Adds positive charge, and are found inside the nucleus of an atom. These are constant, as well. Equal to atomic number.

Front 7

Neutrons

Back 7

Particles with no charge in the nucleus. Equal to protons and atomic number.

Front 8

Electrons

Back 8

Negatively charged; found outside of the atom circulating. These are always moving, and equal to protons in a neutral atom.

Front 9

Bohr Model

Back 9

Planetary model; Electrons orbit the nucleus. Electrons are more stable the closer it is to the nucleus, and there are three levels. The firs three can contain 2, 8, and 8. All lower levels must be filled first.

Front 10

Atomic Mass

Back 10

Total number of neutrons and protons. It is the average of all known isotopes in an element.

Front 11

Mass Number

Back 11

Total number of protons and neutrons in an atom. It is atomic mass rounded off.

Front 12

Isotope

Back 12

Atoms of the same element that contain different numbers of neutrons. These occur during nuclear reactions that cause them to gain or lose neutrons.

Front 13

Ions

Back 13

Elements that have a charge (negative or positive). These are created by losing or gaining electrons. Bonding of metals and non metals.

Front 14

Polyatomic Ions

Back 14

When atoms join, they usually form neutral compounds. Compounds with charge are called this. These gain or lose electrons for a full valence shell.

Front 15

Molecular Compounds

Back 15

These share electrons to form an octet. This is bonding between non metals.

Front 16

Valence Shells

Back 16

These are energy levels that gradually move outwards, away from the nucleus. All elements want a full valence shell called an octet. Metals want to lose electrons, and non metals want to gain.

Front 17

Combining Capacity

Back 17

Measure of the number of covalent bonds that it will need to form a stable molecule.

Front 18

Prefixes

Back 18

When there is only one element in the first name, these are not used. The ending of the second becomes 'ide'. We use these to name molecular compounds:
mono - 1
di - 2
tri - 3
tetra - 4
penta - 5
hexa - 6
septa - 7
octo - 8
nano - 9
deca - 10

Front 19

Non Metals

Back 19

These are typically gases, and are 15% of the Periodic Table. Hydrogen can be this, and a metal. There is no luster, are brittle, and are non conductors.

Front 20

Metals

Back 20

75% of the Periodic Table contains this. The properties of these are luster (shine), silver-grey (gold and copper are exceptions), malleable, ductile, and can conduct heat/electricity.

Front 21

Metalloid

Back 21

Makes up about 10% of the Periodic Table. On the staircase between metals and non metals (B, Si, As, Te, At, Sb, Po). Some have luster, and behave more like metals in their physical properties. They are semi-conductors.

Front 22

Alkali Metals

Back 22

In the first column of the periodic table, each has one electron in its valence shell. These are the most reactive metals, and are always naturally found with other elements. Hint: its like a green LoL champ who is a ninja.

Front 23

Alkaline Earth Metals

Back 23

Column 2. Not as reactive as Column 1 elements. Has two valences. Hint: Basic World.

Front 24

Chalcogens

Back 24

Column 16. Are not as reactive as the other one that sounds like it. Needs two electrons for a full valence shell.

Front 25

Chemical Equation

Back 25

A written representation of a chemical reaction using chemical formulas. Word equations use words and skeleton equations use symbols and formulas.

Front 26

Conservation of Mass

Back 26

This law states that in a chemical reaction, the total mass of the reactants is always equal to the total mass of the products, therefore, equations must be balanced with coefficients. If there is a subscript to brackets, it applies to the brackets.

Front 27

Halogens

Back 27

Column 17. Most reactive non metals. Requires one more electron to be stable.

Front 28

Synthesis

Back 28

Chemical reaction in which the elements combine
H₂ + 0₂ => H₂0 (note that oxygen and hydrogen is diatomic)

Front 29

Decomposition

Back 29

Reaction where elements separate, or break down.
H₂0 => H₂ + 0₂

Front 30

Single Displacement

Back 30

When one element replaces another in the product.
X + YZ => Y + ZX
Mg + 2AgNO₃ => 2Ag +Mg(NO₃)₂

Front 31

Double Displacement

Back 31

When two elements switch places.
WX + YZ => YX + WZ

Front 32

Combustion

Back 32

Reaction where a gas and water is created as a result.
C₆H₁₂O₆ => 6C + 6H₂O

Front 33

Acid/Base

Back 33

Double displacement. One always starts with hydrogen, and the other ends with hydroxide. Can also be called neutralization. The product is always water and a salt by hydrogen reacting with the hydroxide. Concentration L in molarity (M).
Molarity = Moles/L

Front 34

Acids

Back 34

Properties of this are sour tasting, soluble in water, good conductor of electricity, corrosive, reactive and hydrogen ions separate in water. Examples are:
HC₂H₃O (acetic acid vinegar)
HC₆H₇O₇ (citric acid)
HC₆H₇O₆ (ascorbic acid - vitamin C)
HC₃H₅O (lactic acid, sour milk. Causes sore muscles)
H₂CO₃ (carbonic acid - pop)
H₂C₉H₇O₄ (acetyl salicylic acid - ASA, aspirin)
H₂SO₄ (sulfuric acid - car batteries)

Front 35

Bases

Back 35

Properties of this are bitter, soluble in water, slippery in water, good conductor of electricity, hydroxide dissolves with water, and is sometimes called akaline. Examples:
NaOH (Sodium Hydroxide - drain cleaner)
KOH (Potassium Hydroxide - soap, cosmetics)
AlCOH₃ (Aluminum Hydroxide - antacids)
NH₄OH (Ammonium Hydroxide - Windex)
NaHCO₃ (Sodium Bicarbonate - baking soda)
K₂SO₃ (Potassium Sulfite - food preservatives)

Front 36

pH Scale

Back 36

Used to determined how acidic or basic a solution is. pH means power of Hydrogen, or the concentration of hydrogen in a solution. Acids have a low pH value (<7) and bases have a high pH value (>7). Strong acids are from 0-3, and strong bases are 11-14.
pH - -log[H+]
Hydrogen ion concentration, and is measured in moles/L

Front 37

Dalton's Theory

Back 37

Billiard Ball Model. Atoms were thought to be indestructible, inseparable.