Structure bonding and properties

Question 1

What is the nucleon number?

Answer 1

The number of protons and neutrons make up the nucleon number/mass of atom

Question 2

What is the atomic number also known as?

Answer 2

Proton number

Question 3

Define electronic configuration.

Answer 3

Electronic configuration is the arrangement of electrons in an atom

Question 4

Define ions

Answer 4

Ions is an atom or a group of atoms having charge

Question 5

Define octet

Answer 5

octet states that an atom has a tendency to have 8 electrons in the outermost shell

Question 6

Duplet

Answer 6

Helium, Lithium, Beryllium and Boron tend to have 2 lectrons in there outermost shell

Question 7

Chemical bonding

Answer 7

The interaction between varoius atoms to form compounds

Question 8

Ionic bonding

Answer 8

When atoms bond by gaining and losing electrons

Question 9

Covalent bonding

Answer 9

Whenatoms bond by sharing electrons

Question 10

Give examples of ionic and covalent

Answer 10

• covalent
  F2, H20, NH3, CH4, CO2
• Ionic
  NaCl, CaCl2, KI

Question 11

Subatomic particles responsible for recativity

Answer 11

electrons

Question 12

Defne the term lattice.

Answer 12

Lattice is a repetitive sequence or a 3D arrangement of ions atoms in a substance or space

Question 13

Ionic properties of structure

Answer 13

• A giant lattice structure, strong electrostatic forces between oppositely charged ions, high melting and boiling point, conducts electricity in molten or aqueous solutions

Question 14

How do ionic structures conduct electrocity in molten/aqueous solutions?

Answer 14

Ionic bonds are joined by strong electrostatic forces of attraction, so when in contact with molten aqueous solutions, this force is overcome , and the charges are free to move. This allows the charges to conduct electricityhence, defining the property, ionic bonds can conduct electricity in molten/ aquous solutions

Question 15

What are the types of covalent bonds?

Answer 15

Simple and giant

Question 16

Why do simple covalent bonds have such a low melting point?

Answer 16

This is because, the molecules have very weak intermolecular forces of attraction between them, therefore they require less energy to break

Question 17

What is the state of ionic and simple covalent bonds at room temperature?

Answer 17

Simple covalent- gaseous; Ionic covalent is solid

Question 18

Why do ionic bonds have a high melting point?

Answer 18

This is because they have a huge network and a giant lattice structure of oppositely charged ions, which are also joined by electrostatic forces of attraction. The strong electrostatic force forces require a lot of energy to break; therefore, ionic bonds have a high melting point.

Question 19

Properties of simple covalent bonds

Answer 19

Opposite to that of giant covalent bonds

Question 20

Examples of giant covalent bonds

Answer 20

Silicon dioxide, Diamond and Graphite

Question 21

Which substances have covalent bonds?

Answer 21

covalent bonds, as compounds are usually present in a bond of two nonmetals

Question 22

Why is graphite used as a lubricant?

Answer 22

The intermolecular forces of attraction between the layers are very weak, so the hexagonal sheets of graphite can slide over each other easily, making it slippery, hence a great lubricant

Question 23

Why is graphite a good conductor of electricity?

Answer 23

In graphite, each carbon atom is bonded to three other crabon atoms. 1 electron is free to move. This makes Graphite a good conductor of electricity

Question 24

Why does diamond have such a high melting point?

Answer 24

Diamond is arranged in a huge terahedral structure and has a giant network of atoms. These bonds require a lot of energy to break; therefore, diamond has a high melting point

Question 25

Why is diamond an insulator?

Answer 25

Diamond is an insulator as each carbon atom is bonded to 4 others, so there are no free electrons present to conduct electricity.

Question 26

How does mettalic bonding work?

Answer 26

Mettalic bonding is when positive metal ions, arranged in parralell layers, are present in a sea of delocalised electrons; the electrostatic forces attraction created between the electrons and the positive ions make the mettalic bond

Question 27

Why do metals have high melting points and strength?

Answer 27

Metals have high melting points, as there are great electrostatic forces of attraction , which require a lot of energy to break between fixed positive ions and moving delocalised electrons.

Question 28

Properties of metals:

Answer 28

Malleable, ductilemetal are arranged in layers, so they can slide over other very easily

Question 29

What is the generic equation for group 1 reaction with water

Answer 29

2M+ 2H20--------> 2MOH + H2

Question 30

What is the generic equation for group 1 reaction with HCL

Answer 30

2M +2HCL ----> 2MCl +H2

Question 31

What is the generic equation for group 2 reaction with water

Answer 31

M + 2H20-------> 2M(OH)2 +H2

Question 32

What is the generic equation for group 1 reaction with HCL

Answer 32

M +2HCL ----> 2M(Cl) 2 +H2

Question 33

Why are group 1 metals increasing in reactivity as they go down the group?

Answer 33

As we go down the group, the radius and orbits of the elements get bigger, therefore the nucleus has less control over the electron in the last shell. As we go down the group, the more readily the electron is lost.

Question 34

Why are group 1 metals more reactive than group 2?

Answer 34

This is because, group two metals have 2 electrons in their outermost shell, which requires more energy to lose than group 1 elements, which have 1 electron in their outermost shell.

Question 35

Write down all group 1 and group 2 reactions

Answer 35

Grp 1 : Lithium- in water lithium fizzes slowly and eventually disappears - no flame. In HCL lithium fizzes and forms LiCl , and , it will form a red flame Sodium- Sodium fizzes fast in water and melts into a ball, disappearing after some time and may ignite as a yellow/ orange flame. In HCL is does the same but more violently and may produce heat, and makes NaCl Potassium- In water, potassium fizzes rapidly and produces a lilac flame and may explode, and does so in HCL too , but it may ignite into a lilac flame, and produced LiCl Rubidium - In water Rubidium fizzes, explodes a bit after contact and ignites into a red or purple flame before disappearing and in HCL is explodes and ignites, and forms RbCl Cesium- In water Cesium explodes vigorously in contact with the water, and burns into a crimson flame. Same with HCL except it forms CsCl Rubidium- most violent- almost unrecordable Grp 2: (no flame in water in any of them) Beryllium- completely un-reactive Magnesium- In water, it reacts faster with steam, in HCL it fizzes , dissolves, and produces MgCl2 , and ignites into a white flame Calcium- Calcium slowly reacts with cold water to form a slightly cloudy solution with CaOH2, and in HCL it fizzes and forms CaCl2 and produces H2- it ignites in a brick red flame Strontium- in water it reacts a bit faster than calcium and becomes cloudy- it fizzes a bit vigorously and ignites into a crimson flame in HCL Barium- In water barium fizzes vigorously and becomes strongly alkaline , and in HCL it vigorously form BaCl2 and ignites into a pale green flame Radium- most reactive and almost unrecordable (radioactive)- crimson flame in HCL