PART 1: MATTER

CHEMISTRY:

The scientific study of the composition, structure,

properties, and changes in matter.

MATTER:

Anything that has a mass and volume

PARTICLE THEORY OF MATTER:PARTICLE THEORY OF MATTER:

1. All matter is made up of tiny particles.

2. All particles of one substance are the same.

3. Different substances are made of different particles.

4. Particles are always moving. (The more energy, the

faster they move)

5. There are attractive forces between particles. (Forces

are stronger when particles are closer together)

- Any substance or substances

with mass that takes up space.

- Contain two or more

different particles

- Can be physically

separated

- Can only be

chemically

changed

- Contains only one

type of particle

- Particles contain only

one type of atom

-Particles contain

2+ different atoms

- 2+ different

particles , constant

composition

- 2+ different particles

variable composition

PARTICLE DRAWINGS

Pure substance:

element

Pure substance:

molecules of an

element

HON17 or

HOFBrINCl

Pure substance:

molecules of a

compound

Mixture of 2

elements and 2

compounds

1-B

2-C

3-E

4-D

5-A

6-B

7-A

8-E

9-C9-C

10-E

11-B

12-D

13-D

14-D

15-D

Group/Family

o alkali metals

o alkaline earth metals

o transition metals

o other metals

o metalloids

2. Highlight AND LABEL the location of each Group/Family on the mini periodic table below USING A DIFFERENT COLOUR FOR EACH:

o metalloids

o halogens

o noble gases

o Other non-metals

o Lanthanides

o Actinides

Properties of Metals

Properties of Non-metals

Properties of Metalloids

-Shiny

-Malleable

-Hard

-Solid (except

mercury) at

-Dull

-not easily

molded

-Brittle

- solid, liquid, or

-Have

properties of

both metals

and nonmetals

- Semi-

3. Complete the following:

mercury) at

room temp

-Good

conductors of

electricity

- solid, liquid, or

gas at room

temp

-Poor

conductors of

electricity

- Semi-

conductors

(good for

computer

chips)

ParticleRelative

MassRelative Charge

Location within Atom

Proton 1 amu Positive (+) nucleus

Electron 0.00054 amu Negative (-)outside of

nucleus

. 4. Compare the following and label the diagram of the atom below:

Neutron 1 amu Neutral (o) nucleus

nucleus:

protons &neutrons

orbitals:

electrons

Fill in the blanks on calculating the number of subatomic Fill in the blanks on calculating the number of subatomic particles in an atom:

STANDARD ATOMIC NOTATION Atomic number = number of protonsMass number = number of protons + number of neutronsNumber of neutrons = mass number - atomic numberNumber of electrons = number of protons (in a neutral atom)Number of electrons = number of protons + charge (in an ion)

Standard

Atomic Notation

Name of Element

Atomic Number

Mass Number

(Rounded)

Number

of Electrons

Number

of Protons

Number

of Neutrons

Carbon 6 12 6 6 6

Sulphur 16 32 18 16 16

Use the above rules to fill in the table:

Sulphur 16 32 18 16 16

2+ Zinc 30 65 28 30 35

Calcium 20 40 18 20 20

33- Nitrogen 7 14 10 7 7

7. When drawing Bohr-Rutherford diagrams,

follow the pattern below in figure 1.

Figure 2: A completed Bohr-Rutherford diagram for potassium.

Figure 1: Fill energy levels with electrons according

to the pattern shown in this iagram.

# of Electrons= atomic # # of Electrons= atomic # (neutral atom)

# electrons= 15

Place them in each energy level (shell) using the 2, 8, 8 rule, and the clock positions.