Chemistry 10-Alberta Curriculum

Solids

A state of matter in which the object has a definite shape and volume.

Liquids

Definite volume, no definite shape

Gas

A state of matter with no definite shape or volume

Matter

Anything that takes up space and has mass

Heterogeneous Mixture

A mixture in which different materials can be distinguished easily

Physical change

A change in a substance that does not involve a change in the identity of the substance

Chemical change

A change in matter that produces one or more new substances/change into entirely new substance

Malleability

Ability to be rolled into sheets

Ductility

Ability to be stretched into thin wires

Democritus

Greek philosopher that said all matter is made of tiny particles called "atomos" or atoms

Aristotle

All matter is made of four elements: earth, air, fire, water

Dalton's Atomic Theory Billiard Ball

1) elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together 4) atoms only change when mixed with other elements

J.J Thomson

Discovered the electron, plum pudding model

Rutherford

Gold foil experiment, discovered nucleus

Bohr Model

Model of the atom in which electrons move rapidly around the nucleus in paths called orbits (electron shells)

Atomic Number

The number of protons in the nucleus of an atom

Mass Number

The total number of protons and neutrons in the nucleus of an atom

Number of neutrons=

mass number - atomic number

Louie de Brogile

(electron cloud model) Electrons exist in definite energy levels whose exact locations of electrons is uncertain

Periods

Horizontal rows on the periodic table

Families/groups

Vertical columns on the periodic table

Alkali Metals

Group 1

Alkali Earth Metals

Group 2

Halogens

Group 17

Noble Gases

Group 18

Alkali Metals (properties)

Combine with nonmetals, not found in nature, reactive with water and air, silver, soft, melting points lower than the boiling point of water

Alkali Earth Metals (properties)

Silvery-white metals, fairly reactive

Halogens (properties)

Most reactive nonmetals, react with metals to form salts, rarely found in nature,

Noble Gases (properties)

Least reactive, stable because of 8 valence electrons

Transition Metals (properties)

-High melting and boiling points

-Good conductors of electricity and heat

-Strong

-High densities

Metalloids (properties)

Lie on either side of the staircase, share properties with both metals and non-metals

Valance Electrons

The number of electrons in the outermost energy level

Cation

Positive charged ion

Anion

Negative charged ion

Energy level 1 holds how many electrons?

2 electrons

Energy level 2 holds how many electrons?

8 electrons

Energy level 3 holds how many electrons?

18 electrons

Period number of atom =

Number of energy levels occupied

Group number of atom =

Number of valence electrons

Electron dot diagram (aka Lewis structures)

A shorthand representation of the valence electrons in an atom.

Ionic Compounds

Compounds composed of cations and anions

Properties of ionic compounds

Form crystal lattices, conduct electricity in solution, and have high melting and boiling points.

Naming ionic compounds

The name of the metal comes first, followed by the name of the nonmetal, changing the nonmetal's ending to "ide".

Polyatomic ions

Charged composed of one or more elements that act as a single ion together

Naming Polyatomic Ions

Those that contain oxygen usually end with -ite or -ate

-ate has one more oxygen atom

-ite has one less oxygen atom

Multivalent Ionic compounds

Compounds that contain cations that can have more than one possible charge.

You can only use the drop and cross for what compound?

Ionic Compounds

Naming multivalent ionic compounds

Roman numerals are added after the metals name in brackets

Molecular Compounds

Formed from two or more nonmetals

Molecular Compounds (properties)

Low melting point and boiling points, so typically liquids or gases at room temperature (Because the forces between the molecules are weak).

Prefixes are only used with

Naming molecular compounds

1=

Mono

2=

Di

3=

Tri

4=

Tetra

5=

Penta

6=

Hexa

7=

Hepta

8=

Octa

9=

Nona

10=

Deta

Ph Scale

Measurement system used to indicate an acid or base ph level

Acids

Compounds that form hydrogen ions (1-6)

Bases

Hydroxide ions (8-10)

Neutral on the ph scale =

7

Arrhenius

Defined acids and bases based on their behaviour and properties in water

Arrhenius Acid

Substance that dissolves and releases hydrogen ions H+ (aq) in water

Arrhenius Base

Substance that dissolves and releases hydroxide ions OH- (aq)

Red litmus turns red

Hydrogen ions are present

Blue litmus turns blue

Hydroxide ions are present

Red =

Acid

Blue =

Base

Naming Acids

Are named according to their anions. That ionic suffix is dropped and replaced with a new suffix (and sometimes prefix). For example, HCl has chloride as its anion, so the -ide suffix makes it take the form hydrochloric acid.

Capillary Action

The attraction of the surface of a liquid to the surface of a solid

Intramolecular force

Bonds/attractions WITHIN a compound

Intermolecular force

Bonds/attraction BETWEEN covalent compounds

Properties of water

• strong hydrogen bonds

• high specific heat

• high boiling point

• needs a lot of energy to evaporate

• expands when freezes

Why does water expand as it freezes?

Because polar molecules arrange themselves in a more organized, open pattern of hydrogen bonding

High melting and boiling point

Requires lots of energy to break hydrogen bonds to separate the molecules

High specific heat capacity

Absorb energy in the form of heat for a given increase in temperature

Endothermic Reaction

A reaction that ABSORBS energy in the form of heat

Exothermic Reaction

A reaction that RELEASES energy in the form of heat

Law of conservation of energy

the law that states that energy cannot be created or destroyed but can be changed from one form to another

Evidence of chemical reaction

Odor change, color change, formation of a gas, formation of a solid

Closed System

Exchange of energy but no matter

Open System

Exchange of energy and matter

Isolated System

Exchange of neither energy or matter

Law of conservation of mass

The total mass of the reacting substance is always equal to the total mass of the resulting substances

Location of the Proton

Inside the nucleus

Location of the Neutron

Inside the nucleus

Location of the Electron

Outside the nucleus

Charge of the proton

Positive P+

Charge of the neutron

Neutral

Charge of the electron

Negative N-

Mass of Proton and Neutron

1.67 x 10^-27

Mass of the Electron

9.11 x 10^-31

Mole

the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12

Avogadro's number

6.02 x 10^23

Amadeo Avogadro

Proposed the unit mole

Calculate M

Molar mass