Types Of Bonding/ Particles

Question 1

What happens to SOLID particles when the temperature increases and reaches melting point?

Answer 1

heating a solid causes Solid Particles to gain kinetic energy, and vibrate faster.

when temp reaches melting point, the particles use the heat energy to break the forces between them and start melting into a liquid.

Question 2

Explain each particle (solid, liquid, gas) and what happens in each state

Answer 2

Solid: fixed shape and volume, held together by very strong forces. Arranged and Close to eachother. Vibrate in place.
Liquid: fixed volume, no fixed shape. Randomly arranged but close. Slide over eachother.
Gas: no fixed volume, no fixed shape. Randomly arranged and far apart. Very weak forces between particles causing particles to move quickly in all directions.

Question 3

What happens to LIQUID particles when temperature increases and reaches boiling point?

Answer 3

When temp increases, particles start to gain kinetic energy and move FASTER and FURTHER APART.

when temp reaches boiling point, particles use all heat energy to break the forces between them and turn into gas.

Question 4

What type of force holds the oppositely charged ions together in an IONIC BOND?

Answer 4

Electrostatic force

Question 5

Why do group 1 and group 7 elements react with eachother?

Answer 5

Group 1 elements are alkali metals and all react with the nonmetals in group 7 to form ionic compounds.

Gp 1 elements have one e in their outer shell. Gp 7 have 7 electrons in their outer shells. To get full stable shells of 8 electrons each Gp1 readliy give their outer electron to Gp 7 elements

Question 6

What happens during the ionic bonding between gp 1 and gp 7?

Answer 6

The gp 1 elements lose one electron to the gp 7 so that gp 1 can form a full outer shell, the gp 7 elements gain an electron to also form a full outer shell.

Gp 1 elements form a positive ion when losing an electron.
Gp 7 elements form a negative ion when gaining an electron.

Question 7

What happens when atoms lose or gain electrons?

Answer 7

They form ions.

Question 8

State for each of the below whether they form between metals,nonmetals.
Ionic bonding, Covalent bonding, metallic bonding.

Answer 8

1- ionic bonding form between metals and non metals
2- Covalent bonding form between 2 non metals
3- metallic bonding form between 2 metals

Question 9

How are metallic bonds different from ionic and covalent bonds?

Answer 9

In metallic bonds, the electrons are free (delocalized) since the electron had very weak attraction between the positive nucleus which caused it to be free. While in ionic bonds the elements share electrons, and in covalent bonds elements transfer electrons.

Question 10

Why are metals malleable?

Answer 10

Layers of atoms can slide over eachother.

Question 11

How is metallic bonding good conductors of electricity?

Answer 11

Due to the delocalized electrons that are free to move around and carry the current.

Question 12

When do ionic compounds conduct electricity, and why?

Answer 12

When ionic compounds are solid, their ions are in a fixed lattice, so can’t flow. However, when molten or aqueous, the ions are free to move and carry charge.

Question 13

What 3 types of substances can covalent bonds make?

Answer 13

Polymers (chain of molecules strung together)
Giant covalent structures
Simple molecular substances

Question 14

Give 3 examples of giant covalent structures.

Answer 14

Silicon dioxide, diamond, graphite

Question 15

Describe the bonding in simple molecular substances.

Answer 15

There are strong covalent bonds between the atoms of each molecule, but weak intermolecular forces between the different molecules.

Question 16

Why do simple molecular substances have low melting and boiling points?

Answer 16

the intermolecular forces between the molecules are weak, so only require a small amount of energy to break. Which means they can break in low temperatures.

Question 17

Describe the structure and bonding of diamond.

Answer 17

Giant covalent lattice structure.

Each carbon is covalently bonded to 4 other carbon atoms, forming a repeating lattice.

Question 18

Can graphite conduct electricity? Explain why.

Answer 18

Graphite is a good conductor of electricity. Because graphite contains delocalized electrons which are free to move around and carry charge.

Question 19

State the definition of an alloy and how is it stronger than a pure metal-

Answer 19

An alloy is a mixture of a metal and another element; steel could be an alloy since it contains iron and carbon

The different elements have different-sized atoms. (Carbon is a different size and iron is a different size)
This distorts the regular layered structure.
Meaning the layers can’t slide over one another anymore.
This makes alloys stronger

Question 20

State the definition of a metal and how it is weaker than an alloy-

Answer 20

A substance with high electrical conductivity, which lose electrons to form cations.(positive ions)

Metals contain atoms of the same size
Atoms can slide over eachother
Metal is soft, making it weaker.

Question 21

State the definition of nano particles, it’s key features and it’s uses-

Answer 21

Nano particles are very small particles.

Key features: large surface area to volume ratio (as things get smaller the volume decreases rapidly than their surface area)

Uses- ~To deliver drugs around the body
~Nanoparticles can be infused into surgical masks and wounds.
~ nanoparticles can be used in electrical circuits, since some of them can conduct electricity, so they can create tiny computer chips.

Question 22

Issues with nanoparticles-

Answer 22

Nanoparticles are relatively new, not much research has been done. Effects on our bodies aren’t fully understood.

Question 23

State the physical properties of diamond-

Answer 23

Diamond does not conduct electricity-
There are no delocalized electrons that are free to carry a charge/current.

Diamond has a high melting point-
Giant covalent structure
Strong covalent bonds between these carbon atoms which requires high energy to break those bonds leading to HMP.

Extremely hard and dense-
Each carbon atom bonds with 4 other carbon atoms, forming a repeating lattice, leading to a hard structure.

Question 24

State the properties of graphite-

Answer 24

Graphite can conduct electricity-
Each carbon atom forms 3 strong covalent bonds with 3 other carbon atoms, leaving one free electron per carbon atom.
This delocalized is able to move between the layers to carry a charge.

Graphite has a high melting point-
Giant covalent structure
Strong covalent bonds between the carbon atoms

Graphite is soft and slippery-
Although there is strong covalent bonds between the carbon atoms, there are weak intermolecular forces between the layers, causing the layers to be able to slide over eachother, leading to graphite being soft and slippery.

Question 25

Compare between metals and alloys-

Answer 25

Metals-
Contains only one element
Contain Atoms of the same size
Atoms slide over eachother
Soft, weaker than alloys.

Alloys-
Contains a mixture of elements
Contain atoms of different sizes
Not able to slide over eachother easily
Which makes alloys harder and stronger than a pure metal