C3.1 - Everything in the Specification

Question 1 of 16

1

Fill the blank spaces to complete the text.

Originally, John , and then Dmitri , ordered elements by their , because particles had not been discovered.

Explanation

Question 2 of 16

1

Why is it known as the 'periodic' table?

Select one of the following:

Because the properties of the elements show a periodic pattern.
Because it was arranged in six periods by Newlands.
Because it was arranged in six periods by Mendeleev.
Because it was the name coined by 20th-century chemists.

Explanation

Question 3 of 16

1

Fill the blank spaces to complete the text.

' attempt at classifying the was known as the Law of . He noticed that every element had similar , and so he listed the elements in rows of . These were his ''.

However, ' work was criticised by the Chemical Society in 1865, because:
- His groups contained elements that didn't have similar .
- He didn't leave any for to be discovered.
- He mixed up m and .

Explanation

Question 4 of 16

1

Fill the blank spaces to complete the text.

improved on ' work in 1869. He arranged the elements in order of (like ), but he left in order to keep elements with the same in the same vertical . These meant that he predicted elements such as gallium and germanium.

Explanation

Question 5 of 16

1

Scientists only recognised the importance of the periodic table after Newlands' work.

Select one of the following:

True
False

Explanation

Question 6 of 16

1

Fill the blank spaces to complete the text.

When were discovered in the late century, the was arranged in order of the atomic () number of the elements, and all the elements were placed into . The elements can be seen as being arranged by their .

Explanation

Question 7 of 16

1

What property do elements in the same group have?

Select one of the following:

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

Explanation

Question 8 of 16

1

Select from the dropdown lists to complete the text.

The ( positive, negative, neutral ) charge of the ( nucleus, protons, neutrons, electrons ) attracts ( electrons, ions, energy levels, other elements ) and holds them in place - the further away they are, the ( weaker, stronger, more variable ) the attraction. If there are lots of ( inner electrons, protons in the nucleus, neutrons in the nucleus, energy levels ), they get in the way of the ( nuclear, subatomic, negative ) charge, further reducing the attraction. This effect is known as '( shielding, blocking, interception, electron absorption, ion absorption )'.

Explanation

Question 9 of 16

1

The Group 7 metals get more reactive as you go down the group.

Select one of the following:

True
False

Explanation

Question 10 of 16

1

The Group 1 metals get more reactive as you go down the group.

Select one of the following:

True
False

Explanation

Question 11 of 16

1

Fill the blank spaces to complete the text.

The combination of increased and increased means that an electron in a energy level is easily, as there is less attraction from the . Thus, Group metals are reactive as you go down the group.

The combination of increased and increased also means that an electron in a energy level is easily, as there is less attraction from the . Thus, Group metals are reactive as you go down the group.

Explanation

Question 12 of 16

1

Properties of the ❌ (Group 1):

- They get ❌ as you go down the group.
- Their melting and boiling points ❌ as you go down the group.
- They have a ❌.
- They have one ❌.
- They form ❌ compounds with ❌.
- They react with ❌ very vigorously to produce ❌.

Drag and drop to complete the text.

low density

high density

low volume

high volume

Alkali Metals

Transition Metals

Halogens

more reactive

less reactive

smaller

larger

decrease

increase

stay constant

outer electron

inner electron

subatomic particle

ionic

covalent

metallic

electrostatic

non-metals

metals

water

oxygen

flourine

hydrogen

hydrogen gas

chlorine gas

oxygen gas

nitrogen gas

Explanation

Question 13 of 16

1

Properties of the ❌ (Group 7):

- They get ❌ as you go down the group.
- Their melting and boiling points ❌ as you go down the group.
- They all exist as ❌.
- They form ❌ bonds with ❌.
- They can ❌ less reactive halogens from an ❌ of that halogen's ❌.

Drag and drop to complete the text.

Halogens

Alkali Metals

Transition Metals

less reactive

more reactive

smaller

larger

increase

decrease

remain constant

diatomic molecules

subatomic molecules

single molecules

stable ions

ionic

covalent

metallic

electrostatic

metals

non-metals

displace

reduce

oxidise

react with

aqueous solution

aqueous distillation

crystallisation

salt

oxide

halide

Explanation

Question 14 of 16

1

Complete the table showing the properties of different halogens.

Drag an answer into the correct orange point.

Flourine

Bromine

Iodine

Yellow

very reactive

Dark red

poisonoud

reactive

dense

Purple

crystalline

Explanation

Question 15 of 16

1

Properties of the Transition Metals (Middle of the Table):

- They conduct ❌.
- They are very ❌, ❌ and ❌.
- They are ❌ than Group1 metals.
- They are much ❌, ❌ and ❌ than the Group 1 metals.
- They have ❌ melting and boiling points than the Group 1 metals.
- They often have more than one ❌.
- Their compounds are often ❌.
- They all make good ❌.

Drag and drop to complete the text.

heat and electricity

heat

electricity

dense

voluminous

reactive

strong

brittle

shiny

matte

less reactive

more reactive

denser

less dense

stronger

weaker

harder

softer

much higher

much lower

very similar

ion

charge

particle

colourful

ionic

catalysts

insulators

building materials

Explanation

Question 16 of 16

1

What is the charge on a halide when it forms an ionic compound?

Select one of the following:

1-
1+
2-
2+
Neutral

	Created by Harry Woodhall over 7 years ago

A quick quiz on everything outlined in the C3.1 specification.

C3.1 - Everything in the Specification

Question 1 of 16

Fill the blank spaces to complete the text.

Originally, John , and then Dmitri , ordered elements by their , because particles had not been discovered.

Explanation

Question 2 of 16

Why is it known as the 'periodic' table?

Select one of the following:

Explanation

Question 3 of 16

Fill the blank spaces to complete the text.

Explanation

Question 4 of 16

Fill the blank spaces to complete the text.

improved on ' work in 1869. He arranged the elements in order of (like ), but he left in order to keep elements with the same in the same vertical . These meant that he predicted elements such as gallium and germanium.

Explanation

Question 5 of 16

Scientists only recognised the importance of the periodic table after Newlands' work.

Select one of the following:

Explanation

Question 6 of 16

Fill the blank spaces to complete the text.

When were discovered in the late century, the was arranged in order of the atomic () number of the elements, and all the elements were placed into . The elements can be seen as being arranged by their .

Explanation

Question 7 of 16

What property do elements in the same group have?

Select one of the following:

Explanation

Question 8 of 16

Select from the dropdown lists to complete the text.

Explanation

Question 9 of 16

The Group 7 metals get more reactive as you go down the group.

Select one of the following:

Explanation

Question 10 of 16

The Group 1 metals get more reactive as you go down the group.

Select one of the following:

Explanation

Question 11 of 16

Fill the blank spaces to complete the text.

Explanation

Question 12 of 16

Properties of the ❌ (Group 1): - They get ❌ as you go down the group. - Their melting and boiling points ❌ as you go down the group. - They have a ❌. - They have one ❌. - They form ❌ compounds with ❌. - They react with ❌ very vigorously to produce ❌.

Drag and drop to complete the text.

Explanation

Question 13 of 16

Properties of the ❌ (Group 7): - They get ❌ as you go down the group. - Their melting and boiling points ❌ as you go down the group. - They all exist as ❌. - They form ❌ bonds with ❌. - They can ❌ less reactive halogens from an ❌ of that halogen's ❌.

Drag and drop to complete the text.

Explanation

Question 14 of 16

Complete the table showing the properties of different halogens.

Drag an answer into the correct orange point.

Explanation

Question 15 of 16

Drag and drop to complete the text.

Explanation

Question 16 of 16

What is the charge on a halide when it forms an ionic compound?

Select one of the following:

Explanation

Properties of the ❌ (Group 1):

- They get ❌ as you go down the group.
- Their melting and boiling points ❌ as you go down the group.
- They have a ❌.
- They have one ❌.
- They form ❌ compounds with ❌.
- They react with ❌ very vigorously to produce ❌.

Properties of the ❌ (Group 7):

- They get ❌ as you go down the group.
- Their melting and boiling points ❌ as you go down the group.
- They all exist as ❌.
- They form ❌ bonds with ❌.
- They can ❌ less reactive halogens from an ❌ of that halogen's ❌.