C2 Flashcards
What area of the periodic table are the metals found in
Left
What area of the periodic table are the non metals found in
Right.
Rows are called…
Columbs
Vertical columns are called…
Groups
What does the group number tell you about the element
How many electrons the have in their outer shell
What type of ion do metals form when they react
Positivte ion
What do atoms generaLly react to form
A full outershell
What type of bond do metals have
Mettalic bond
What does a metallic bond cause metals to have
A similar basic physical propeties
What are metals great at
Conducting heat and electricity
What are group 1 elements know as
Alkali metals
What elements are in group 1
Lithium, sodium, pottasium, rubidium, caesium and francium
How many electrons do group 1 elements contain in their outershell and what does this mean
They all have 1 electron in their outershell meaning this makes them very reactive and have similar properties.
What are some properties of group 1 elements
Soft, low density
Trends in group 1
- as you go down, increase in reactivity - as you go down, the electron gets further away from nucleus meaning the attraction between nucleas decreases
- meaning lower melting points and boiling points as you go down
- higher relative atomic mass as you go down
What ion do alkali metals form
+1 ion
What happens when alkali metals react with water?
They react vigorously. More reactive as you go down. Lithium pottasium sodium float and move around whilst fizzing vigourously. They also produce hydrogen
What is produced when reacted with chlorine
White salts called metal chlorides.
What happens when alkali metals react with oxygen
They form metal oxide.
Lithium = lithium oxide
Sodium = sodium peroxide & sodium oxide
Pottassoum = pottassium peroxide & pottassium superoxide
What are group 7 elements known as
Halogens
Halogens and their appearence
Fluorine - very reactve, poisonous yellow gad
Chlorine - fairly reactive, poisenous dense green gas
Bromine - dense, poisonous red-brown volatile liquid
Iodine - dark grey crystalline solid or a purple vapour
Trends of halogens
As you go down…
Less reactive - harder to gain an extra electron as further away from nucleus
Higher melting and boiling points
Higher relative atomic masses
How many electrons are in halogens outer shell
7
What can halogens form to get a full outershell?
Molecular compounds: share electrons via covalent bonding with other non metals. The compounds which form all have a simple-molecular structure
What ion do halogens form
1- ion called halides when they react with metals. These all have ionc structures
In halogens, how can a displacement reaction occur?
When a more reactive halogen reacts with a salt of the less reactive one
What are group 0 elements called
Noble gases
How many electrons do noble gases have in their outer shell and what does this mean
8 meaning they are extremely unreactive as they have a full outershell
What are noble gases all?
Inert colourless gases.
What do noble gases exist as
Monatomic gases
What are the patterns in properties in noble gases!
Boiling points Increase as you go down.
How do you find out the trend in reactivity in a group in the period table?
If the elements are trying to lose 1 or more electrons, the reactivity will increase because as the electrons get further away from the nucleus, it is easier to lose the electron. But if the elements are trying to gain, the reactivity decreases as it is harder to gain electrons as the electrons are further away from the nucleus
What does electrostatic attraction depend on?
-the distance between the outermost electrons and the nucleus
-the number of occupied inner shells of electrons which have a shielding effect
-the size of the positive charge on the nucleus
What to factor to decide how easy it is for atoms to lose or gain electrons from their outershell?
-the increased nuclear charge
-due to extra protons in the nucleus
Problems with categorising elements in the 1800s:
-scientists had no idea of atomic structure or of protons
-only thing you could measure was atomic weight
Why did mendaleev leave gaps?
To make sure thst elements with similar properties stayed in the same group. Some of these groups indicated the existence of undiscovered elements
What did the discovery of isotopes confirm?
That mendaleev was correct not to place elements in a strict order of atomic weight but to also account for their properties
Physical properties of metal?
-strong and can be bent or hammered
-great at conducting heat and electricity
-high melting and boiling points
Non-metal physical properties?
-dull looking
-brittle
-low density
-dont conduct electricity
