P1. Topic 1- Atomic Structure And The Periodic Table

Question 1

How many elements are there

Answer 1

118 known elements.

Question 2

Where are the elements listed

Answer 2

The periodic table

Question 3

What are compounds

Answer 3

Substances made from two or more elements chemically bonded

Question 4

How can conpounds be separated into their elements

Answer 4

Chemical reactions

Question 5

What is a mixture

Answer 5

Two or more substances that are not chemical bonded

Question 6

Why isn’t distillation a chemical process

Answer 6

No new substances are made, it is a separation technique

Question 7

Describe John Dalton’s model of the atom

Answer 7

Atoms are solid spheres that cannot be divided

Question 8

Describe the plum pudding model

Answer 8

Atoms are one ball of positive charge with negative electrons embedded within the structure

Question 9

What did James Chadwick do, and why was it significant

Answer 9

Discovered the neutron, explaining the missing mass in the atom

Question 10

What is an atom

Answer 10

The smallest part if an element that can still be identified as that element

Question 11

What experiment led to the discovery of the nucleus?

Answer 11

The alpha particle scattering experiment.

Question 12

How did Niels Bohr adapt the nuclear model?

Answer 12

He suggested that electrons orbit the nucleus at specific distances.

Question 13

How large is an atom?

Answer 13

About 0.1 nanometres (1 x 10^-10 metres).

Question 14

What proportion of the atom is its nucleus?

Answer 14

The nucleus is tiny - around 1/10,000 of the atom’s diameter.

Question 15

What does the atomic number of an element tell you?

Answer 15

The number of protons.

Question 16

What does the relative atomic mass of an element tell you?

Answer 16

The average mass of an atom, taking into account its isotopes.

Question 17

Name the three sub-atomic particles.

Answer 17

Protons, neutrons, electrons.

Question 18

Give their relative charges.

Answer 18

Proton: +1, Neutron: 0, Electron: -1.

Question 19

Give the relative masses of the subatomic particles

Answer 19

Proton: 1, Neutron: 1, Electron: ~0 (very small).

Question 20

Which particles are found in the nucleus?

Answer 20

Protons and neutrons.

Question 21

Why do atoms have no overall charge?

Answer 21

Because they have equal numbers of protons and electrons.

Question 22

How do you calculate the number of neutrons in an atom?

Answer 22

Relative atomic mass - atomic number.

Question 23

What are isotopes?

Answer 23

Atoms of the same element with different numbers of neutrons.

Question 24

Where are electrons found in the atom?

Answer 24

In energy levels (shells) around the nucleus.

Question 25

When drawing atoms, where should the first electrons be placed?

Answer 25

In the first shell, closest to the nucleus.

Question 26

How many electrons can fit in the first shell?

Answer 26

2 electrons

Question 27

How many electrons can fit in the second shell?

Answer 27

8 electrons

Question 28

What is the maximum number of electrons you should draw in the third shell?

Answer 28

8 electrons (for GCSE purposes).

Question 29

What are elements arranged in order of in the modern Periodic Table?

Answer 29

Increasing atomic number.

Question 30

What are the columns (of the Periodic Table) called?

Answer 30

Groups

Question 31

What are the rows (of the Periodic Table) called?

Answer 31

Periods

Question 32

Where are the metals found?

Answer 32

On the left and towards the bottom of the Periodic Table.

Question 33

What do elements in the same Group have in common?

Answer 33

They have the same number of electrons in their outer shell.

Question 34

Why is the table called 'Periodic'?

Answer 34

Because properties of elements repeat at regular intervals.

Question 35

What were elements in early Periodic Tables placed in order of?

Answer 35

Atomic mass.

Question 36

Why was this different to the system we use now?

Answer 36

Now we use atomic number which better matches properties.

Question 37

Why were early Periodic Tables incomplete?

Answer 37

Because not all elements had been discovered.

Question 38

What was novel about Dmitri Mendeleev's Periodic Table?

Answer 38

He left gaps and predicted properties of undiscovered elements.

Question 39

Why did scientists adopt Mendeleev's table?

Answer 39

Because his predictions were later proven correct.

Question 40

What other name do Group 1 go by?

Answer 40

The alkali metals

Question 41

Why are the alkali metals named like that

Answer 41

They form alkaline solutions when they react with water.

Question 42

What does lithium make when it reacts with water?

Answer 42

Lithium hydroxide and hydrogen gas.

Question 43

How do you test for the two products? (Hydrogen and hydroxide)

Answer 43

Hydrogen: 'squeaky pop' test (DO NOT write squeaky pop on exam paper- you will not be credited) with a lit splint. Hydroxide: Use universal indicator - turns purple/blue.

Question 44

What do the atoms of lithium, sodium and potassium have in common?

Answer 44

They all have one electron in their outer shell.

Question 45

Describe how reactivity changes as you go down Group 1.

Answer 45

It increases

Question 46

Explain why the reactivity changes down group 1

Answer 46

Outer electron is further from the nucleus and more easily lost.

Question 47

How does the reaction of potassium with water look different to lithium?

Answer 47

Potassium reacts more violently - lilac flame, more fizzing.

Question 48

Why are Group 1 metals kept in oil?

Answer 48

To prevent them reacting with oxygen and moisture in the air

Question 49

How do Group 1 metals react with chlorine?

Answer 49

They form white salts (metal chlorides).

Question 50

Compare the physical properties of the Group 1 metals to the transition metals.

Answer 50

Group 1 are softer, less dense, have lower melting points and are more reactive.

Question 51

Explain why the Group 1 metals are soft.

Answer 51

They have weaker metallic bonding.

Question 52

What other name do Group 7 go by?

Answer 52

The Halogens.

Question 53

What do the atoms of fluorine, chlorine and bromine have in common?

Answer 53

They all have seven electrons in their outer shell.

Question 54

Describe how reactivity changes as you go down Group 7.

Answer 54

It decreases

Question 55

Why does reactivity decrease as you go down Group 7.

Answer 55

The outer shell is further from the nucleus, so it's harder to gain an electron.

Question 56

Describe what form Group 7 elements are found in.

Answer 56

As diatomic molecules (e.g., Cl2).

Question 57

Describe and explain the trend in boiling point as you go down Group 7.

Answer 57

Boiling point increases due to stronger intermolecular forces.

Question 58

What other name do Group 0 go by?

Answer 58

The Noble Gases

Question 59

What do the atoms of helium, neon and argon have in common?

Answer 59

They have full outer electron shells.

Question 60

Describe the impact of this on their chemical reactions.

Answer 60

They are unreactive.

Question 61

Describe and explain the trend in boiling point as you go down Group 0.

Answer 61

Boiling point increases due to greater intermolecular forces.

Question 62

Where in the Periodic Table are the transition metals?

Answer 62

In the centre block (between Groups 2 and 3).

Question 63

Give four typical properties of these metals.

Answer 63

High melting points, dense, strong, good conductors.

Question 64

Give three chemical properties that are particular to the Transition Metals.

Answer 64

Form coloured compounds, have variable oxidation states, act as catalysts.

Question 65

Explain why many of the transition metals are used to make jewellery.

Answer 65

They are shiny, unreactive, and strong.

Question 66

What is an isotope

Answer 66

Same number of protons and electrons but different neutrons

Question 67

What is an ion

Answer 67

Same amount of protons and neutrons but different amount of electrons.