Periodic table

Question 1

What are the vertical columns in the periodic table called?

Answer 1

-The vertical columns in the periodic table are called groups. First seven groups are numbered 1 to 7 and the final group is numbered 0

Question 2

What are the elements in orange called?

Answer 2

Transition metals

Question 3

What is group 1 called?

Answer 3

Alkali metals

Question 4

What is group 7 called?

Answer 4

Halogens

Question 5

What are group 0 called

Answer 5

Noble gases

Question 6

What are the horizontal rows in the periodic table called?

Answer 6

-The horizontal rows in the periodic table are called periods. It is important to remember that hydrogen and helium make up Period 1

Question 7

What are elements in the periodic table in arranged in order of?

Answer 7

-Elements are arranged on the periodic table in order of increasing atomic number each element has one more proton than the element preceding it. This is done so hat elements end up in columns with other elements which have similar properties.

Question 8

What are groups?

Answer 8

-Groups are vertical columns that show how many outer electrons each atom has and are numbered from 1-7 with the final group being 0 for example each group 4 element has 4 electrons on its outer shell so will need to lose 4 o complete a full outer shell were as a element in group 6 has 6 electrons on its outer shell so will need to gain 2 to make 8 a full outer shell…

Question 9

What are the two numbers against each element symbol?

Answer 9

Most periodic elements have two numbers against each symbol or element. The atomic number will always be the smaller number. The other number will be the mass number or the relative atomic mass

Question 10

What is the number of protons in an atom represented by?

Answer 10

Atomic number

Question 11

What is the number of electros equal to

Answer 11

the number of protons (atomic number)

Question 12

What is the number of neutrons in an atom?

Answer 12

mass number - atomic number

Question 13

What do reactions in elements depend on?

Answer 13

-The reactions of atoms depend on how many electrons there are in their outer shell. These are the electrons which normally get involved when elements bond to other elements. Elements in the same group have the same number of electrons in their outer shell therefore they react in similar ways.

Question 14

What are the noble gases?

Answer 14

-Group 0 elements are also known as the noble gases because they are almost completely unreactive, in fact the two at the top of the group helium and neon do not react with anything. The elements in group 0 have 8 electrons in their outer hell apart from helium which has 2 The lack of reactivity of the elements in group 0 is associated with their electronic configurations. The noble gases are unreactive because their outer shell is full so their is no tendency to lose, gain or share electrons in a chemical reaction.

Question 15

Where are the metals and non metals in relation in the periodic table

Answer 15

-The metals are on the left hand side of the periodic table and the non metals are on the right hand side.

Question 16

What are the properties of metals

Answer 16

-Metals conduct electricity and non-metals do not generally conduct electricity. The reasons that metal conduct electricity is due to the presence of delocalised electrons because the electrons are free to move and pass on the current. -Metals generally form basic oxides A basic oxide is one which reacts with acids to form salts for example copper to copper (II) oxide.-Tend to be solids with high melting an boiling points, and with relativity high densities
-Are shiny when they are polished or cut
-Are malleable can be hammered or changed into shape
-Are ductile
-Are good conductors of electricity and heat
-Form ionic compounds
-Form positive ions in their compounds

Question 17

What are the properties of the non metals

Answer 17

-Non metals do not conduct electricity because there are no free electrons that are free to move or ions there are a few exceptions like graphite
-Non metals genreally form acidic oxides acidic oxides react with bases/ alkalis to form salts-Tend to have low melting and boiling points
-Tend to be brittle when they are solids
-Dont usually conduct electricity some exceptions like graphite
-Are poor conductors of heat of heat diamond is an exception best conductor f heat of all elements
-Form both ionic and covalent compounds
-Tend to form negative ions in ionic compounds

Question 18

What happens when going down the group for metals?

Answer 18

melting and boiling point goes down.

Question 19

What are the properties of the alkali metals?

Answer 19

Melting and boiling points of the elements are very low for metals and get lower as you move down the group.
Their densities tend to increase down the group, although not regularly. Metals are very soft and easily cut with a knife becoming softer as moving down the group shiny and silver when freshly cut tarnish quickly when exposed to air.

Question 20

What do metal react with oxygen to form?

Answer 20

form oxides

Question 21

What happens when Group 1 metals react with oxygen or water vapour?

Answer 21

extremly reactive so reactive that they have to be stored in sealed glass tubes to stop possibility of oxygen getting to them

Question 22

What are the properties of Group 1 metals?

Answer 22

One electron on their outer shell. All react with water. All react with oxygen to form an oxide they form ionic compounds

Question 23

Explain the water reaction with sodium

Answer 23

When water reacts with sodium there are clear observations. The sodium floats because it is less dense than water. The sodium melts into a ball because its melting point is low and a lot of heat is produced by the reaction. There is fizzing because hydrogen gas is produced. The sodium moves around on the surface of the water. because the hydrogen is not given off symmetrically around the ball the sodium is pushed around the surface of the water. The sodium gets smaller and disappears sodium is used up. Test the solution with universal indicator goes blue , indicating an alkaline solution has been formed metal hydroxide is alkaline

Question 24

Explain the water reaction with Lithium

Answer 24

Fizzes and floats. The reaction is very similar to sodium’s reaction, its a much slower reaction. As lithium’s melting point is higher and the heat produced is not as quick so it does not melt.

Question 25

Explain the water reaction with Potassium

Answer 25

Potassium’s reaction is faster than sodium’s heat is produced to ignite the hydrogen which burns with a lilac flame. The reaction often ends with the potassium spitting around and exploding it fizzes and floats.

Question 26

Explain the water reaction with Rubidium

Answer 26

React even more violently than potassium can be explosive rubidium hydroxide and caesium hydroxide are formed.

Question 27

Explain the increase in reactivity in groups

Answer 27

As you go down the group metals become more reactive. Difference between the reactions depend on how easily the outer electrons of the metal is lost. depends on how strongly it is attracted to the nucleus in the atom. As moving down the group the atoms have more shells of electrons and get bigger As the atom gets bigger the outer electron the one lost in the reaction is futher from the nucleus because it is further from the nucleus so less attracted.

Question 28

Explain the reaction of the Alkali metals with O2

Answer 28

Lithium sodium and potassium are all stored in oil because they react with the air.

Question 29

Explain what happens when lithium is heated and reacts with air

Answer 29

Lithium burns with a red flame

Question 30

Explain what happens when sodium is heated and reacted with air

Answer 30

Sodium burns a yellow flame to form sodium oxide

Question 31

Explain what happens when Potassium is heated and reacted with air

Answer 31

Potassium burns with a lilac flame to form potassium oxide.

Question 32

What is the equations for these reactions?

Answer 32

4M(s) + O2 > 2M2O

Question 33

What are the compounds of the Alkali metals?

Answer 33

All group 1 metal ions are colourless. This means that their compounds will be colourless or white unless they are combined with a coloured negative ion. Group 1 compounds are typical ionic solids and are mostly soluble in water

Question 34

Summarise the main features of the Group 1 elements

Answer 34

-Are metals
-Are soft with melting points and densities which are very low for metals
-Have to be stored out of contact with air and water
-react with water to produce an alkaline solution of the metal hydroxide ad hydrogen gas
-Increased reactivity as going down
-Form compounds in which the metal has a +1 ion
-have mainly colourless compounds which dissolve to produce colourless solutions

Question 35

What are some examples of halogens?

Answer 35

chlorine, bromine, Florine

Question 36

What are halogens?

Answer 36

Elements that have 7 electrons in their outer shell. All group 7 elements react in a similar way

Question 37

What happens when halogens react with metals?

Answer 37

produce a wide range of salts like calcium fluoride silver bromide. Also known as halides

Question 38

Why do melting and boiling points increase down the group in halogens?

Answer 38

Halogens are all covalent molecular substances and the melting and boiling point increases as the relative molecular mass increases. As it increases the intermolecular forces of attraction become stronger and therefore more energy is required to overcome the strong forces of attraction. no covalent bonds are broken.

Question 39

Why are halogens poor conductors of heat and electricity

Answer 39

Non metals no delocalised electrons to pass on the current

Question 40

What are the safety problems with all of the halogens?

Answer 40

Extremly poisonous vapours liquid bromide very corrosive