Major Ideas: Atoms & Periodic Table

Question 0

• protons
  1. Charge
  2. Location
  3. Identification
  4. Function

Answer 0

1. Positive (+1)
2. Nucleus
3. Atomic number
4. Distinguishes element

Question 1

What are the three ‘things’ atoms are composed of?

Answer 1

• protons
• neutrons
• electrons

Question 2

• Neutrons
  1. Charge
  2. Location
  3. Identification
  4. Function

Answer 2

1. Neutral (0)
2. Nucleus
3. Mass number minus proton number
4. Determines isotope

Question 3

• Electrons
  1. Charge
  2. Location
  3. Identification
  4. Function

Answer 3

1. Negative (-1)
2. Orbiting/moving around nucleus
3. Proton number
4. Reactivity

Question 4

What makes an atom electrically neutral?

Answer 4

Number of protons and number of electrons are equal

Question 5

What are isotopes?

Answer 5

Atoms of the same element that have different numbers of neutrons in the nucleus

Question 6

What are ions?

- 2 different types

Answer 6

Ions are charged atoms

• positive ions: more protons than electrons
• negative ions: more electrons than protons

Question 7

What are valence electrons?

Answer 7

Electrons in the outermost ‘shell’ of an atom

Question 8

What are the similarities between elements in the same group?

Answer 8

Same number of number of valence electrons

Question 9

What are the similarities between elements in the same period?

Answer 9

Same number of valence shells

Question 10

What are the similarities between elements in transition metals?

Answer 10

Same colour in solution

Question 11

What is ionisation energy?

Answer 11

Energy required to remove the most ‘loosely’/first electron bound in an atoms (gaseous state)

Question 12

What cause ionisation energies to increase?

Answer 12

• charge of ion is increased

- electron is removed from shell closer to nucleus

Question 13

What is first ionisation energy?

Answer 13

Amount of energy required of remover FIRST electron

Question 14

What effect does the electron distance from nucleus have on the first ionisation energy??

Answer 14

The further away the less amount of electrostatic force has to be overcome hence it is more easily removed. If it is closer to the nucleus the electrostatic force is much stronger hence more energy is required to overcome the force; increasing f.i.e

Question 15

What effect does the number of electrons compared to protons have on first ionisation energy?

Answer 15

The more positive charge (protons) the stronger the electrostatic attraction, hence making the electron more difficult to remove

Question 16

How do you determine core charge?

Answer 16

Subtract the number of inner-shell electrons from the number of protons

Question 17

Periodic trend: atomic radius

- why?

Answer 17

Increases down the group and decreases across the period

- more number of electrons = stronger electrostatic force of attraction, pulls valence shell closer

Question 18

Periodic trend: first ionisation energy

- why?

Answer 18

Decreases down the group and increases across the period

• further away from the nucleus as you go down the group
• smaller atomic radius resulting in a stronger electrostatic force (high f.i.e)

Question 19

What is electronegativty?

Answer 19

Measure of electron-attracting power of an atom in a molecule
- pull an electron to itself

Question 20

Periodic trend: electronegativty

- why?

Answer 20

Decreases down the group and increases across the period

• closer to nucleus and smaller radii
• reactivity