C2 The Periodic table🧩

Question 1

How made the first attempt of the periodic table in the 19th century?

Answer 1

John Dalton

Question 2

In what year did John Dalton produce his ‘table of elements’?

Answer 2

1808

Question 3

How built on Daltons idea in 1864?

Answer 3

John Newlands

Question 4

How did Dalton order his elements?

Answer 4

He ordered them by there atomic weights.

Question 5

What did Newlands assume when created his ‘table of octaves’? And what mistake did he make?

Answer 5

He assumed that all existing elements had already been discovered. And he filled in his octaves even though some were not similar at all

Question 6

How did Newlands order his elements?

Answer 6

He ordered them by their mass with the properties of every eighth element being similar ( however we know this only worked for a few)

Question 7

Who built on Newlands idea in 1869?

Answer 7

A Russian chemist called Dmitri Mendeleev.

Question 8

How did Mendeleev arrange the elements?

Answer 8

He placed them in order of their atomic mass. He then arranged the table so that a periodic (regularly occurring) pattern in their properties could be seen.

Question 9

What did Mendeleev do that Newlands didn’t?

Answer 9

He left gaps in his table for elements that were yet to be discovered.

Question 10

What made other scientists believe Mendeleev?

Answer 10

The predictions he made about where other elements would fit in were correct, this meant he was able to get other chemists to believe in him.

Question 11

What problem did Argon cause for Mendeleev?

Answer 11

Argon atoms had a greater relative mass than potassium atoms. Ordering by atomic weights meant Argon (a noble gas) was in a group with reactive metals like sodium and lithium. And potassium (a EXTREMELY reactive metal) was with completely unreactive noble gasses. He couldn’t group it with the noble gases because they had not been discovered.

Question 12

What did Mendeleev do about elements being in a group with very different properties?

Answer 12

He simply just changed the order of elements to keep ones with similar properties in the same group.

Question 13

In the 20th century, how were elements finally ordered?

Answer 13

Eventually, scientists found out elements had to be ordered by their atomic numbers (amount of protons in each atom).

Question 14

What are the vertical columns called in the periodic table?

Answer 14

They are called groups.

Question 15

What are the horizontal lines in the periodic table called?

Answer 15

These are called periods.

Question 16

What do elements in the same groups all have in common?

Answer 16

All elements in the same group will react in similar ways as they all have the same amount of electrons in there outer most shell.

Question 17

How many electrons will group 2 elements have in their outer most shell?

Answer 17

2 electrons.

Question 18

What is one difference between metals and non-metals?

Answer 18

Metals conduct electricity but non-metals are electrical insulators - a notable exception being some forms of carbon. Metals also tend to have much higher melting and boiling points.

Question 19

What is an ion?

Answer 19

An ion is a charged atom or a charged group of atoms.

Question 20

What type of ion will elements in group 5,6,7 form.

Answer 20

They will form negative ions. This is because they gain electrons to fill their outer shells. Therefore having more electrons than protons, making it negative. These then have the electronic structure of the noble gas at the end of the period

Question 21

What type of ion will group 1,2,3 elements form.

Answer 21

They will form positive ions. This is because they will loose electrons in their outer shell. As they lose electrons to do this, they will become positively charged as they have more protons than electrons. These then have the electronic structure of the noble gas at the end of the period

Question 22

How many electrons do group 0’s have in their outer shell?

Answer 22

They will all have a full shell of 8 electrons in their outermost shell meaning that they are very stable. However, Helium only has 2 in its outer shell. As it only has 2 electrons, this still fills the first shell, making it very stable along with the rest of group 0.

Question 23

Why do group 0’s tend not to react.

Answer 23

They don’t need to react with anything as they already have a full outer shell and don’t need to modify their electronic structure by forming molecules.

Question 24

Are the boiling points of group 0 higher at the top or bottom of group 0?

Answer 24

The boiling points get higher as you down the group. Helium (He) at the top boils at -269°C, where as at the bottom radon (Rn) boils at -62°C.

Question 25

Give yourself a break, you’ve been studying for a while!

Answer 25

Im joking carry on revising you lazy child

Question 26

What is another name for the group 1 metals

Answer 26

They are also known as the alkali metals.

Question 27

What elements are in group 1?

Answer 27

Lithium
Sodium
Potassium 
Rubidium
Caesium
Francium

Question 28

How reactive are group 1 metals.

Answer 28

VERY reactive

Question 29

Is the reactivity highest at the top or bottom of group 1?

Answer 29

The most reactive metal (Francium) is at the bottom of the group 1 metals.

Question 30

Why do group 1 metals have to be stored in oil?

Answer 30

Otherwise they would react with oxygen in the air.

Question 31

Why do some group 1 metals float on water?

Answer 31

This is because their density is lower than waters.

Question 32

Why does the shiny silver layer disappear soon after you cut into them?

Answer 32

This is because they are reacting with oxygen and a layer of oxide forms. For example, forming sodium oxide.

Question 33

Why are group one metals so reactive?

Answer 33

They only need to lose one electron in there outer shell to become stable meaning they will react with non-metals to make this happen.

Question 34

What happens as you go down group 1?

Answer 34

B.P and M.P decrease, elements get softer and reactivity increases

Question 35

What happens when you add lithium, sodium or potassium to water?

Answer 35

They float and fizz violently on the water. Potassium actually forms a lilac flame and sodium a golden yellow one when it reacts because the hydrogen produced ignites. They also produce a hydroxide (OH) which is soluble in water and why they are called the alkaline metals (hydroxides are alkaline). This means if you put universal indicator in after the reaction it would turn purple (alkaline).

Question 36

What is the word & symbol equation for sodium + water?

Answer 36

Sodium (or which ever group one is asked for) + water -> sodium hydroxide + hydrogen
2Na + 2H(sub script)2O -> 2NaOH + H(sub script) 2

Question 37

What colour is the solution when Group 1’s react with water?

Answer 37

The solution is actually colourless (haha trick question)

Question 38

What is another name for the group 7 elements?

Answer 38

These elements are also known as the halogens.

Question 39

Are group 7 elements non-metals?

Answer 39

Yeah they are

Question 40

What happens as you go down the halogens?

Answer 40

M.P and B.P increase and reactivity decreases

Question 41

What elements are in group 7?

Answer 41

Fluorine
Chlorine
Bromine
Iodine
Astatine

Question 42

Do group 7’s conduct electricity well?

Answer 42

Nope

Question 43

What is the bond called that pairs up the group 7 atoms to make them molecules? Why do they have to bond?

Answer 43

A covalent bond. They are diatomic (unstable on its own). NOTE: if you are asked to write the symbol equation for anything to do with halogens remember when no in a compound they have a 2 next to them.

Question 44

How many electrons do the halogens need to gain to have a full outer shell.

Answer 44

1 electron.

Question 45

Are group 7 metals reactive.

Answer 45

Yes, they are reactive as they only need to gain one electron to have a full outer shell.

Question 46

Name an example of a group 7 reacting with a metal.

Answer 46

Sodium Chloride (others may be correct)

Question 47

What happens if a more reactive halogen is added to a less reactive halogen in a salt?

Answer 47

The more reactive halogen would displace the less reactive halogen from solutions of its salt. e.g chlorine + potassium bromide - potassium chloride + bromine

Question 48

What colour is Chlorine in solution?

Answer 48

Pale green

Question 49

What colour is Bromine in solution?

Answer 49

It will be yellow

Question 50

What colour is Iodine in solution?

Answer 50

Darker red/brown

Question 51

What would happen if you had chlorine + potassium bromide?

Answer 51

Chlorine + Potassium bromide -> Potassium chloride + Bromine

Question 52

What halogen has the ability to replace all the others?

Answer 52

Fluorine as it’s the most reactive.

Question 53

What happen to the electron structure every time you go down an element in a group?

Answer 53

An extra electron shell gets added.

Question 54

What effect does having more shells have on an atom?

Answer 54

Larger atoms lose electrons more easily going down the group. Larger atoms gain electrons less easily as you go down the group.

Question 55

Why is it harder for big atoms to gain electrons?

Answer 55

The outer shell if further from the nucleus (where the protons are) so the magnetic pull to attract other electrons won’t be as strong. The inner shells of the electrons ‘shield’ the force from getting to the other electrons further out.

Question 56

Why does the reactivity increase the lower down you go in group 1?

Answer 56

The further from the nucleus your are the easier it will be to lose that one extra electron in the outer shell. This is because the electron is further from the attractive force of the protons in the nucleus. So when you gain a shell every time you go down a period, the attraction to keep the extra electron will decrease.

Question 57

The positive charge does increase the more electrons you have as there is also more protons. So why doesn’t the attraction for the outer shell get stronger?

Answer 57

The distance from the nucleus and the shielding effect simply outweigh the effect of the extra protons.

Question 58

Why does reactivity decrease in group 7 electrons the further down the group you go?

Answer 58

At the top, there are less electrons in the way so it is easier for the protons to attract in one more electrons. However, at the bottom of the group, the distance from the outer shell to the nucleus is further. As the attraction is weaker, it is harder to attract a extra electron, making them less reactive.

Question 59

Where are the transition metals positioned?

Answer 59

They are positioned in the middle of Group 2 and group 3.

Question 60

What are the physical properties of transition metals?

Answer 60

They are good conductors of electricity.
They are hard and strong
They are quite dense
They have high melting points.

Question 61

What are more reactive, group 1 metals or transition metals?

Answer 61

Group 1 metals are a lot more reactive than group 1 metals. This means they don’t do things like reacting so fast with oxygen.

Question 62

Why are transition metals often used for construction?

Answer 62

This is because they don’t react with many things, meaning that they are very safe to work and build with. And all their physical properties are also useful

Question 63

What colour compound does copper form?

Answer 63

Blue

Question 64

What colour compound does nickel form?

Answer 64

Pale green

Question 65

What colour compound does Chromium form?

Answer 65

Dark green

Question 66

What colour compounds do manganese form?

Answer 66

Pale pink

Question 67

What colour does any compound of the alkaline metals turn

Answer 67

White e.g slat

Question 68

What colour does any halogen compound change to?

Answer 68

Can vary depending on what it is reacting with (doesn’t decide the compounds colour)

Question 69

What does the roman number near transition metals mean? And why does it have it?

Answer 69

It has it because it can from different ions eg Fe2+ or Fe3+. And the numeral means how many more electrons it has (II = 2+). The different ions of the same element can form different coloured compounds. Eg iron (II) gives green compounds by iron(III) gives a reddish brown.