Vce Chemistry 1 Chapter 1

Front 1

The kinetic theory of matter

Back 1

• Particles of different substances have different sizes.
• Lighter particles move faster than heavier ones at a set temperature.
• Particles move faster at higher temperatures
• Solids: particles are very close and vibrate in fixed positions
• Liquids: particles are further apart, have more energy and they can move around each other.
• Gasses: particles are far apart, move rapidly and randomly

Front 2

Volatile

Back 2

Liquids that evaporate at a low temperature.

Front 3

Ion

Back 3

Formed when an atom loses or gains an electron and becomes charged

Front 4

Isotope

Back 4

An atom of an element with a different number of neutrons than protons and hence a different mass number. Similar chemical properties because number of electrons are the same. Different physical properties because their masses differ.

Front 5

Z

Back 5

Atomic Number = number of protons

Front 6

A

Back 6

Mass Number = number of protons and neutrons

Front 7

Compound

Back 7

A pure substance composed of different elements chemically joined together in fixed proportion by mass.

Front 8

Element

Back 8

A pure substance containing only atoms with the same number of protons. Atoms have an equal amount of protons and electrons and thus a neutral charge

Front 9

Mixture

Back 9

Formed when two or more pure substances are mixed without chemically reacting.

Front 10

Period Number

Back 10

Number of shells that contain electrons = number of shell containing the valence electrons.

Front 11

Valence Electrons

Back 11

The electrons in the outermost shell containing electrons.

Front 12

Electron Configuration

Back 12

Describes the arrangement of electrons in energy levels (or shells) around the nucleus.

Front 13

Electron shells

Back 13

Electrons can be visualised as moving within a region of space surrounding the nucleus. The regions are called electron shells, labelled K, L, M, N, and numbered 1, 2, 3, 4. A definite energy level is associated with each shell, the one closest to the nucleus, K, being the lowest energy level. An electron has to gain energy to move further away from the nucleus. If it gains enough energy to completely leave the atom, the particle that is left is no longer neutral and is called a positive ion.

Front 14

Formula for maximum number of electrons in a shell

Back 14

2n² where n = number of shell. For first 20 elements the max number of valence electrons = 8.

Front 15

Atomic Emission Spectrum

Back 15

Produced by passing the light emitted by an element through a prism. Atomic emission spectra consist of separate lines of coloured light. Each line in an emission spectrum corresponds to one particular frequency of flight being given off by the atom; therefore each line corresponds to one exact amount of energy being emitted.

Front 16

Periodic Table Groups

Back 16

Columns of the Periodic Table. Each element in a group has the same number of valence electrons.

Front 17

Alkali Metals

Back 17

Group 1. React with water to form alkaline solutions. Very reactive. Low Density.

Front 18

Alkaline Earth Metals

Back 18

Group 2. First extracted from oxides in earth's crust. Less reactive than alkali metals.

Front 19

Halogens

Back 19

Group 17. So reactive that they don't occur freely in nature. Combine with different metals to form salts.

Front 20

Noble/Inert Gasses

Back 20

Group 18. Do not react readily. Exist as single Atoms. Colourless at room temperature with low melting and boiling points.

Front 21

Metalloids

Back 21

AKA Semi Metals. Have properties of both metals and non-metals.

Front 22

Transition Metals

Back 22

Large group of metals from group 3 to 12

Front 23

Periodic Table Periods

Back 23

Rows of periodic table. Elements in a period have their valence electrons in the same electron shell and share a gradual change in chemical and physical properties.

Front 24

Lanthanides

Back 24

Period 6. Rare earth metals.

Front 25

Actinides

Back 25

Period 7. Radioactive Elements.

Front 26

Periodic table trend down a group

Back 26

More electron shells mean bigger atomic size and because outer electrons are shielded by inner shells, they are less attracted to nucleus.

• metallic character increases & non-metallic character decreases
• atomic size increases
• reactivity Increases
• electronegativity decreases

Front 27

Periodic table trend across a period

Back 27

The attraction force of the nucleus increases with increasing number of protons. This pulls the electron shells closer to the nucleus

• metallic character decreases & non-metallic character increases
• atomic size decreases
• reactive at the start of the period, less in the middle and reactive at the end
• fluorine = most electronegative. The further away an element is placed from fluorine in the periodic table, the less electronegative it is.

Front 28

Position of Hydrogen

Back 28

• group 1 (alkali metals) - 1 valence electron that can be lost during reactions
• group 17 (halogens) - share many properties and can gain an electron during reactions
• often placed away from any particular group

Front 29

Atomic Symbol

Back 29