Bonding

Question 1

Metallic- what allows a charge to run through metallic structures?

Answer 1

Delocalised electrons

Question 2

What force holds the structure together?

Answer 2

Electrostatic attraction

Question 3

What are the physical attributes of metallically bonded compounds?

Answer 3

Can conduct electricity, high boiling and melting points, are malleable and ductile

Question 4

What allows for malleability in metallically bonded compounds?

Answer 4

Uniform arrangement- in a lattice, all the ions are the same size

Question 5

Ionic- What do ionic bonds exist between?

Answer 5

Metals and non-metals

Question 6

What is the direction of electron donation in ionic bonding?

Answer 6

From metal to non-metal

Question 7

When can an ionically bonded compound conduct electricity?

Answer 7

Aqueous state (electrons will be free to move)

Question 8

Why is the boiling point in ionic bonding high?

Answer 8

The electrostatic attraction between the positive and negative ions is strong thus to overcome this bond a lot of energy will be required

Question 9

Why are ionic compounds brittle?

Answer 9

When bonds are moved they repel each other.

Question 10

What is the chemical process used around ionic bonding?

Answer 10

Electrolysis

Question 11

Covalent- what is a dative covalent bond between?

Answer 11

An electron deficient molecule and an electron rich molecule

Question 12

What is covalent bonding?

Answer 12

Shared pair of electrons between two atoms

Question 13

What is electronegativity?

Answer 13

The ability of an element to attract electron density towards itself in a covalent bond

Question 14

What is the trend of electronegativity in periodic table?

Answer 14

Increases up a period and across a group

Question 15

Why are Helium and Hydrogen not electronegative?

Answer 15

They do not form covalent bonds

Question 16

What is a Van der Waals force?

Answer 16

The forces between oppositely charged atoms

Question 17

What causes the difference in charge in atoms?

Answer 17

Unequal distribution of electrons in an atom- temporary dipole

Question 18

What causes induced dipoles in atoms?

Answer 18

When another atom with a temporary dipole approaches another atom causing equal charges to repel.

Question 19

What factors effect the induction of a dipole?

Answer 19

Number of electrons and size/mass of the atom, how close the atoms can get together (branching)

Question 20

when do dipole-dipole forces exist?

Answer 20

When there is a permeant dipole present

Question 21

What do dipole-dipole forces require to exist?

Answer 21

Permanently electronegative elements to create a charge difference

Question 22

What does hydrogen bonding occur between?

Answer 22

Hydrogen, N/O/F

Question 23

What is hydrogen bonding?

Answer 23

When a free pair of electron are attracted towards a d+ hydrogen

Question 24

What is the difference between the densities of water and ice? Why?

Answer 24

Ice is less dense than water due to the H bonds increase in length so to keep the waters bond angles the same.

Question 25

What is ices structure?

Answer 25

H bonds form hexagonal structure which always dissolve in water.

Question 26

What structure does Diamond have and name some properties?

Answer 26

Tetrahedral structure

It has strong covalent bonds, it is a hard material, very high melting point, does not conduct electricity due to no delocalised electrons

Question 27

What structure does Graphite have and name some properties?

Answer 27

Trigonal planar structure

Can create a current as delocalised electrons and a interchangeable double bond.

Infinitely long layers of carbon held together by VDW forces, soft material as layers can slide over each other and high melting point due to covalent bonds