topic 6- groups in the periodic table

What are the group 1 metals known as

Alkali metals

What is the trend in the alkali metals as you go down. Mention there reactivity and their boiling points

Reactivity increases down the group and boiling points decreases

Why does the reactivity increase as you go down the group

Atomic radius is increased. The outermost electron has weaker attraction to the nucleus so is recited with a another atom easier

Why does the boiling points decrease as you go down the group

The metallic bonds become weaker so less energy is needed to overcome the metallic bonds

What are the properties of the alkali metals

Mention there:

How they feel

Their density

Their melting point

And how they react with water oxygen and group 7 elements

Soft

Low density

Low melting points

React vigorously with water oxygen and group 7 elements

What are the products of water reacting with alkali metals

They produce a metal hydroxide and hydrogen gas

What are the products of chlorine gas reacting with an alkali metal

Produce a white metal chloride salt

What are the products of oxygen reacting with a alkali metal

Produces a metal oxide

What are group 7 elements known as

Halogens

What is the characteristics of flourine

A poisonous yellow gas which is very reactive

What are the characteristics of chlorine

A less reactive poisonous green gas

What are the characteristics of bromine

A ready brown volatile liquid

What are the characteristics of iodine

A dark grey solid which can form a poisonous purple vapour and is also an antiseptic which has saved millions of lives

What type of structure do they form with non metals

A simple molecular structure with covelant bonds

What are the trends with the group mention melting and boiling points and their reactivity

Melting and boiling points increase down the group

Reactivity decreases as you go down the group

Why does the reactivity decrease as you go down the group

The outermost shell goes further and further away from the positive nucleus so the attractive force that’s needed to pull in another electron s weaker so its harder to react to gain that electron

How do halogens form ionic bonds with metals

They gain an electron to harm a 1- ion which we call a halide

What is a displacement reaction and give an example

When a more reactive halogen displaces a more reactive halogen in a reaction

Such as chlorine gas and potassium bromide reacting to form iodine gas and potassium chloride

What care group 8 elements known won as

Noble gases

What are their characteristics mention their colour how they react and their flammability and how they come as

They are all colourless gases

These gasses all have full outer shells and are therefore inert

Inert- they don’t really react with anything

Exist as single atoms

Non-flammable

Explain why boiling points increase as you go down the group of noble gases

because there are more electrons in the atoms down the group this increases the attractive forces between the atoms so therefore more energy is required to overcome the forces

give uses to the noble gases

helium

argon

helium- much less dense in air so its used in balloons and is non flammable

argon- filament lamp stops the hot metal filament burning away as it creates a inter atmosphere

welding- shields the hot metal from oxygen in the air

what is observed when lithuim reacts with water

Hydrogen gas bubbles are produced. Lithium floats and moves slowly over the water surface.

What is observed when sodium reacts with water?

Sodium floats and fizzes, moves quickly, then melts into a silvery ball.

What is observed when potassium reacts with water?

Potassium floats, fizzes and moves very rapidly; it melts and burns with a lilac flame, sometimes exploding.