Atomic Structure And The Periodic Table

Question 1

1.State the definition of the following words: atom, element, compound & mixture

Answer 1

1. Atom the smallest part of an element that can exist.
   Element a group of atoms
   Compound a mix of 1 or more types of element not chemically bonded
   Mixture a mix of 1 or more types of element chemically bonded

Question 2

1. Name the four methods of separation
2. Draw and label a diagram of the distillation apparatus
3. Describe and explain how distillation works
4. Draw and label a diagram of the crystallisation apparatus
5. Describe how to carry out crystalisation
6. Describe how to carry out chromatography (REQUIRED PRACTICAL

Answer 2

1. Distillation crystallisation chromatography heating
2. Place your salt water into a beaker. And enter the apparatus into the beaker. Then let the water go up through it and you will then have distilled water at the other end.
3. Place your salt water on a tray on a Bunsen burner. Then gently heat it up. Remove from the heat and let the mixture cook down. Leave in a sunny area for 24hrs and crystal with form which will be table salt
4. Get a sheet of chronograph paper and draw a line of where your water will go up to. Place it on a cocktail stick to keep it level and place it into the water. Wait for it to rise and you will be able to see the levels of acids and alkalis in the mischief

Question 3

1. Describe the ‘plum pudding model’ of the atom?
2. Which experiment led to the plum pudding model being rejected?
3. Describe Rutherford’s scattering experiment and its results
4. What did Rutherford’s “scattering experiment” provide evidence for?
5. What did Niels Bohr discover?
6. What else did Rutherford discover?
7. What did James Chadwick discover?
8. Approximately, what’s the size of an atom?

Answer 3

1. A ball of charge with a positive centre mass and negative electrons embed
2. Rutherfords scattering experiment.
3. Alpha particles were fired at thin sheets of gold. Most went straight through. Some where deflected some where rebounded
4. Centre mass or nucleus
5. That the electrons orbit the nucleus
6. Nucleus
7. Neutrons
8. 0.1 nm

Question 4

1. What are the relative charges on the subatomic particles?
2. Explain why atoms have no overall charge
3. Atoms of the same element have the same number of which subatomic particle?

Answer 4

1. Proton +1 
    Neutron 0
    Electron -1
2. Electrons cancel out protons 
3. Proton

Question 5

1. On the periodic table of the elements, what is the top number called?
2. In terms of subatomic particles, what does the mass number represent?
3. On the periodic table of the elements, what is the bottom number called?
4. In terms of subatomic particles, what does the atomic (or proton) number represent

Answer 5

1. Atomic number
2. Mass number
3. Proton and neutrons
4. Electrons

Question 6

1. What are the relative masses of the subatomic particles?
2. What are isotopes?
3. Describe how carbon-12 is different to carbon-14?

Answer 6

1. Proton 1
   Neutron 1
   Election 1/2000
2. The same element that have equal amounts of proton but different numbers of neutrons in the nuclei
3. Carbon-12 has 2 less neutrons than carbon-14

Question 7

1. What is relative atomic mass?

2. State the equation for calculating the relative atomic mass, if given the abundance of different isotopes

Answer 7

1. The weight of an an atom

2. Ar = total number of atoms/ total number of atoms

Question 8

1. In terms of electron arrangement, what is the maximum number of electrons allowed in the first 4 shells?
2. Draw the electron arrangement for an oxygen atom (atomic number = 8)

Answer 8

1. 2, 8, 8, 8, 8

Question 9

1. By what number are the elements within the periodic table arranged?
2. Why was the Periodic Table given this name?
3. In the Periodic Table, what are the horizontal rows called?
4. In the Periodic Table, what are the vertical columns called?
5. Describe how elements were arranged in the early Periodic Table and the problem that resulted.
6. Why didn’t ordering by atomic weight work very well?
7. What innovation did Mendeleev bring to the layout of the periodic table

Answer 9

1. Atomic
2. Elements appear periodically
3. Groups
4. Rows
5. Atomic weight
6. Gaps
7. Properties

Question 10

1. What are most of the elements in the periodic table?
2. In the periodic table, where are non-metals located?
3. Name 4 properties of metals
4. Name 3 properties of non-metals

Answer 10

1. Non metals
2. Left
3. High melting and boiling point, can conduct electricity and heat
4. Molten or gas at room temperature, can not conduct electricity or heat

Question 11

1. What is another name for the group 1 metals?
2. What is similar about the electron structure of group 1 metals?
3. Describe the properties of group 1 metals
4. Describe the trend in properties as we go down group 1?
5. Explain why group 1 metals are more reactive down the group

Answer 11

1. Alkali metals
2. 1 electron on outer shell
3. Very reactive with air and water, high melting and boiling points, soft
4. 1 electron on outer shell gets further away from nucleus
5. 1 electron on outer shell gets further away from nucleus so easier to loose

Question 12

1. What another name for the group 7 elements
2. What charge do halogens have when they form ions? Why?
3. Describe the trend in properties as we go down the group 7
4. Explain why group 7 elements are less reactive down the group
5. Name the properties of the halogens

Answer 12

1. Halogens
2. Negative they gain electron
3. Atomic radius increases, becomes more difficult to attract
4. Atomic radius increases

Question 13

1. Name the properties of the group 0 elements (Noble gases)
2. Why are the noble gases inert (unreactive)?
3. Describe and explain the change in boiling point of the noble gases as you go down the group?

Answer 13

1. Colourless, odourless, tasteless, non flammable
2. Full outer shell
3. Boiling point increases as the atom gets denser