Atomic Structure and Bonding

Question 1

Where are metals found on the periodic table?

Answer 1

Metals are found under the bold line.

Question 2

Name groups 0, 1 and 7.

Answer 2

Group 0- Noble gasses
Group 1- Alkali metals
Group 7- Halogens

Question 3

Link the number of outer electrons to the group number.

Answer 3

The number of outer electrons of an element matches the group number.

Question 4

What elements have similar chemical properties?

Answer 4

Elements in the same group have similar chemical properties.

Question 5

What are the 3 sub-atomic particles, what’s their charge, mass and where are they found?

Answer 5

Proton
charge= 1+
mass= 1
location= inside the nucleus

Neutron
charge= 0
mass= 1
location= inside the nucleus

Electron
charge= 1-
mass= almost 0
location= in energy levels outside the nucleus

Question 6

Describe the significance of Rutherford’s Gold Foil experiment.

Answer 6

Most of the particles passed straight through the foil without being deflected but occasionally some were deflected. This lead Rutherford to the conclusion that the cause of the deflections were due to the centre of the atom having a positive charge with the rest of the atom being mostly empty space.

Question 7

What’s the atomic number?

Answer 7

The atomic number is equal to the number of protons in the nucleus.

Question 8

What’s the mass number?

Answer 8

The mass number is equal to the number of protons added to the number of neutrons in the nucleus.

Question 9

Why are atoms neutral?

Answer 9

Atoms are neutral because they have an equal number of protons and electrons/positive and negative charges.

Question 10

What is the structure of nuclide notation?

Answer 10

mass number
elements symbol
atomic number

Question 11

What are isotopes?

Answer 11

Isotopes are atoms with the same atomic number and a different mass number.

Question 12

What is a mass spectrometer used to find?

Answer 12

Scientists use a mass spectrometer to find:
- the number of isotopes present
- the mass of each isotope
- the relative proportion of each isotope as a percentage.

Question 13

What is relative atomic mass and where can it be found in the data book?

Answer 13

The relative atomic mass is the average mass of the isotopes in a sample of an element. They are listed on page 7 of the data book.

Question 14

What is an ion?

Answer 14

An ion is a charged atom. They are formed when atoms gain or lose electrons.

Question 15

How do you determine the charge of an ion?

Answer 15

The charge of an ion can be determined by finding the electron arrangement of the element and finding how many electrons need to be gained or lost to reach a stable outer energy level of 8. If the atom needs to gain electrons the charge will be the number of electrons it needs to gain then a -. If the atom needs to lose electrons the charge will be the number of electrons it needs to lose then a +.

Question 16

What types of elements take part in covalent bonding?

Answer 16

non-metal

Question 17

What type of elements take part in covalent bonding?

Answer 17

Non-metals

Question 18

How are covalent bonds formed?

Answer 18

A covalent bond forms when two positive nuclei are held together by their common attraction for a shared pair of electrons.

Question 19

What are the definitions of single, double and triple covalent bonds?

Answer 19

A single covalent bond consists of one pair of shared electrons.
A double covalent bond consists of two shared pair of electrons.
A triple covalent bond consists of three shared pair of electrons.

Question 20

What are the 7 diatomic elements?

Answer 20

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine and iodine.

Question 21

What are the different shapes of molecules?

Answer 21

Linear, angular, trigonal pyramidal and tetrahedral.

Question 22

What are the two types of covalent structures?

Answer 22

Covalent molecular and covalent network.

Question 23

Describe the structure of covalent molecular substances.

Answer 23

Covalent molecular substances are made up of molecules joined together, in the liquid and solid states, by weak forces of attraction called van der Waals forces.

Question 24

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

Answer 24

During melting and boiling it is only the weak forces of attraction that are broken. This process requires little energy so covalent molecular substances have low melting and boiling points.

Question 25

Describe the structure of a covalent network substance.

Answer 25

A Covalent network consists of a giant 3 dimensional network of atoms joined together by strong covalent bonds.

Question 26

Why do covalent networks have high melting and boiling points?

Answer 26

They have very high melting points because the network of strong covalent bonds is not easily broken as lots of energy is needed to break covalent bonds.

Question 27

Why do covalent substances not conduct in any state?

Answer 27

Covalent substances do not conduct in any state as they do not contain any charged particles. Graphite (carbon) is the exception as only three of its outer electrons are involved in bonding, the fourth is free moving or delocalised.

Question 28

Are covalent molecular substances soluble in water?

Answer 28

Some covalent molecular substances are soluble in water whereas some aren’t. This can be found on the table on page 8 of the data book.

Question 29

Are covalent molecular substances soluble?

Answer 29

They do not dissolve in any solvents.

Question 30

How do you tell the state of a substance at room temperature from its melting and boiling point?

Answer 30

If the melting point is above room temperature the substance is a solid at room temperature.
If the melting point is lower than room temperature but the boiling point is higher than room temperature the substance is a liquid at room temperature.
If the boiling point is below room temperature the substance is a gas at room temperature.

Question 31

What does an ion electron equation look like for calcium?

Answer 31

calcium ——–> Ca2+ + 2e-
(metal) ion
2,8,8,2 2,8,8

Question 32

What is an ionic bond?

Answer 32

An ionic bond is the electrostatic attraction between oppositely charged ions.

Question 33

Describe the structure of an ionic compound.

Answer 33

Ionic compounds are made up of metal and non-metal ions joined together by ionic bonds. An ionic substance consists of a lattice structure of oppositely charged ions with each positive ion surrounded by negative ions, and each negative ion surrounded by positive ions.

Question 34

Why do ionic compounds have high melting points?

Answer 34

Ionic compounds have high melting and boiling points because lots of energy is needed to break the strong ionic bonds in the lattice.

Question 35

What happens to the ionic lattice when an ionic compound dissolves in water or is melted?

Answer 35

As they dissolve, the lattice structure breaks up allowing water molecules to surround the separated ions. The ions are now free to move.

Question 36

Why do ionic compounds not conduct as solids but do conduct as liquid and molten?

Answer 36

Ionic compounds do not conduct in the solid state because the ions are not free to move, as they are held rigidly in the crystal lattice by strong ionic bonds. However ionic compounds do conduct when molten or in solution because the ions are free to move. Melting and dissolving breaks up the crystal lattice.

Question 37

What happens during conduction of an ionic solution?

Answer 37

During the conduction of an ionic solution or molten ionic compound, the ions move towards the oppositely charged electrodes. This is called electrolysis.

Question 38

Name the non-metal that is used as electrodes in conductivity apparatus for liquids.

Answer 38

Graphite (carbon)