YEAR 9 – Topic 4 & 5– Ionic, Covalent & Metallic Bonding Flashcards
How are ions formed?
When a metal and non-metal react and the metal atom loses electrons to form a positive ion and the non-metal gains electrons to form a negative ion.
What is the charge of the elements in…
Group 1 – The Alkali Metals?
+
What is the charge of the elements in…
Group 2 – The Alkaline Earth Metals?
2+
What is the charge of the elements in…
Group 3?
3+
What is the charge of the elements in…
Group 4?
No Charge!!!
What is the charge of the elements in…
Group 5?
3-
What is the charge of the elements in…
Group 6?
2-
What is the charge of the elements in…
Group 7 – The Halogens?
-
What is the charge of silver (Ag)?
+
What is the charge of copper (Cu)?
2+
What is the charge of iron (Fe)?
2+ or 3+
What is the charge of lead (Pb)?
2+
What is the charge of zinc (Zn)?
2+
What is the charge of hydrogen (H)?
+
What is the charge and formula of hydroxide?
OH (-)
What is the charge and formula of ammonium?
NH4 (+)
What is the charge and formula of carbonate?
CO3 (2-)
What is the charge and formula of nitrate?
NO3 (-)
What is the charge and formula of sulphate?
SO4 (2-)
What is the bond which occurs between metals and non metals?
Ionic
Explain ionic bonding…
The definition
Electrostatic attraction between oppositely charged ions.
How is an ionic bond formed?
What are the rules?
(5 points)
– The electron(s) on the outer shell can be gained or lost.
– Metals loose electrons to non metals.
– Non metals gain electrons from metals.
– it takes less energy to loose/gain fewer electrons
– The elements become charged ions (+,2+,3+,-, 2-, 3-)
What is the (ionic) formulae for…
Aluminium chloride?
Al = Group 3
Cl = Group 7
Al – charge of 3+ Cl – charge of - So... Al Cl . 3
What is the (ionic) formulae for…
Iron (III) sulfide?
S = Group 6
Fe – charge of 3+ S – charge of 2- So... Fe S . 2 3
What is the (ionic) formulae for…
Magnesium hydroxide?
Mg = Group 2
Mg – charge of 2+ OH – charge of - So... Mg (OH) . 2
What is the (ionic) formulae for…
Potassium carbonate?
K = Group 1
K – charge of + CO3 – charge of 2- So... K CO . 2 3
What is the (ionic) formulae for…
Iron (III) sulfate?
Fe – charge of 3+ SO4 – charge of 2- So... Fe (SO ) . 2 ( 4) . 3
What is the (ionic) formulae for…
Magnesium nitrate?
Mg = Group 2
Mg – charge of 2+ NO3 – charge of - So... Mg (NO ) . ( 3) . 2
What key things do you need to remember when drawing dot and cross diagrams for ionic bonding?
(7 points)
– Only outer shells need to be drawn – Show electron moving across – No overlapping of the electrons When done... – Put square brackets around them – Show their charge (+, 2+, 3+, -, 2-, 3-) – Put the little vertices lines between the two or more elements to sho the movement of electrons. – LIP GIN!!!
What is the bond which occurs between non metals?
Covalent
Explain covalent bonding…
The definition
When the non metals are bonded, they share a pair(s) of electrons. This is because there is an electrostatic attraction between the shared pair electrons and the nuclei.
What key things do you need to remember when drawing dot and cross diagrams for covalent bonding?
(3 points)
– Atoms overlapping
– Show all orbitals unless stated otherwise
– Put the element symbol inside the shells
How is an covalent bond formed?
What are the rules?
(4 points)
– The elements join together and share electrons because of the electrostatic attraction.
– The shared electrons are attracted to the ions.
– One pair of electrons (2 electrons) shared = 1 bond.
– A maximum of 4 bonds can be formed between 2 elements but overall you can have many more bonds.
What is the bond which occurs between metallic elements and alloys?
Metallic
Explain metallic bonding…
The definition
When they are bonded, the electrons become delocalised and move around the structure of ions. They have an electrostatic attraction between the delocalised electrons and the metal ions.
What key things do you need to remember when drawing diagrams for metallic bonding?
(4 points)
– Big ions close together
– Small electrons surrounding the ions
– Ions shown as positive
– Electrons shown as negative
How is an metallic bond formed?
What are the rules?
(4 points)
– The ions join together.
– Their electrons get “ripped” off and become delocalised.
– The electrons move about freely between the lattice (structure) of ions.
– The electrons are attracted to the ions like we are to the earth.
How do you represent a metallic lattice in a 2D diagram?
4 points
– Big ions close together – Small electrons surrounding the ions – Ions shown as positive – Electrons shown as negative (Positive ions surrounded by a sea of delocalised electrons)
