Atoms and the Periodic Table Revision

Flashcards about Atoms and the Periodic Table

Give three properties of typical metals.

Shiny, Good conductor of Electricity, Good conductor of HEAT, malleable, Ductile, mainly Solid @RM Temp

Isotopes

Elements with a different number of Neutrons but the same number of Protons

Compare the trends in reactivity as you move down Group 1, Group 7 and Group 0.

Group I are more reactive going down the Column/group, Group 7 less reactive moving down group, Group 0 or 8 Are NOT Reactive

State three things that increase as you move down Group 1, Group 7 and Group 0.

Atonic number, Atomic mass, Number of Energy levels

Give three properties of typical non-metals.

Dull, Non conductive HEAT, Non conductive Electricity, mostly liquid or Gases @ RM temp

Properties of alkali metals

Solid @ Room Temp, Very reactive in water, Good Conductors, Shiny when Cut, Soft

Properties of halogens

Solid, liquid or gases @ em temp, Very Reactive, Poor conductors, Solids are Brittle

Properties of noble gases

All Gases @em temp, All poor conductors, All Un reactive

Elements in NaCl

Sodium + Chloride

Elements in MgO

Magnesium + Oxygen

Elements in Mgs

Magnesium + Sulphur

Elements in Fes

Iron + Sulphur

1:1

Ratio of elements in CaO

1:1

Ratio of elements in NaCl

1:2

Ratio of elements in MgCl2

1:1

Ratio of elements in lithium fluoride

2:1

Ratio of elements in K₂0

1:1:1

Ratio of elements in NaOH

Compare diamond and graphite.

Both are Covalent Substances. Diamond has 4 Covalent Bonds with 4 other Carbons.. Very hard and do NOT Conduct. Graphite has 3 carbon bonds is flat and has I atom free' so can conduct electricity as it has delocalised electrons and is also a lot softer due to Structure

Why the noble gases are so unreactive.

They have Full Outer Shells

Acid reactions with a metal

A metal reacts with an acid a metal Salt and Hydrogen gas are formed.

Acid reactions with a metal carbonate

When a Metal Carbonate reacts with an acid a metal salt and Water and Carbon dioxide gas is produced.

Why might the mass go down when a gas is produced during a reaction?

Gas released to atmosphere. Reaction vessel is Open

sodium + chlorine →

Sodium Chloride

lithium iodine →

lithium Iodide

potassium + bromine →

Potassium bromide

Equation for when magnesium reacts with oxygen

2Mg +0₂ - 2MgO

How are the groups arranged in the periodic table?

By Their properties

How can you tell that the alkali metals are very reactive?

Only 1 electron in outer Shell

How can you tell the noble gases are unreactive?

Full outer shells

What happens to the mass of the product from the question above?

Mass of Product will be the Same as the mass of Reactants

Mg + O₂ -> MgO

magnesium oxide

Be + S -> BeS

Beryllium Sulphide

Be + F₂ -> BeF

Beryllium Fluoride

2K+ Cl₂ -> 2 KCI

Potassium Chloride

List 3 halogens

Chlorine, lodine, Fluorine, Astatine

How many electrons do halogens have in their outer shell?

7

Describe how the reactivity changes as you go down the group.

Become less reactive as atom is larger harder for Positive Protons to attract them.

bromine + potassium iodide

Br₂ + 2 KI -> 2KB + I₂

chlorine + sodium iodide

Cl₂ +2NaI ->2 NaCl + I₂

Sodium Hydroxide + Hydrochloric acid produces Sodium Chloride and Water.

NaOH + HCI -> NaCl + H₂O

Describe what happens to the reactivity of the alkali metals as you go down the group.

More reactive

Why are alkali metals more reactive down the group?

Outer electron is furthest away from the Positive Protons

Some metals react with acid to produce…

salt and hydrogen