groups in the periodic table Flashcards
(32 cards)
Properties of metal
-high melting and boiling points
-good conductors of heat and electricity
- all solids at room temperature apart from mercury
- form positive ions
where are non metals found on the periodic table and why
on the right side of the table because they have many electrons on their outer shell
properties of non metals
-lower melting and boiling points than metals
-often found as gases
-generaly do not conduct heat or electricity
what is a noble gas
an element found in group 0
why are elements in group 0 unreactive
because they already have a full outer shell so they dont need to gain or lose any electrons to fill it
why are noble gases used in light bulbs
because they wont react with the hot metal filament
Noble gases properties
-low melting and boiling points
-monoatomic
-low density
-Inert (unreactive)
- not flammable
- colourless
what are halogens
elements found in group 7
halogen properties
-7 outer electrons
-diatomic
-form salts
what happens to the reactivity as you go down group 7 and why
- because the atoms gain more electron shells so distance between the outer shell and nucleus increases
- so the attraction between them is weaker , this makes it harder to gain an electron
- outer energy levels are shielded from the positive charge of the nucleus from internal electrons
What are the elements in group 1 called
Alkali metals
what happens to the reactivity as you go down group 1 and why
increases because the attraction between the electron and the positively charged nucleus becomes weaker therefore msking it easier to lose an electron
- there is a greater distance between the positive nucleus and negative outer electron
- the outer electron is shielded from the nucleus by the internal energy levels
where are the transition metals found
in the middle of the table between group 2 and 3
properties of transition metals
-strong and hard
-high melting points
-lower reactivity
-high density
transition metals special properties
-can form more than one ion
-can form coloured compounds
-can be used as catalyst
describe group 1 metals reacting with water
- react vigorously to produce hydrogen gas and metal hydroxides
- as you go down the group, the reaction becomes more violent
- the amount of energy given out by the reaction increases as we go down the group
describe group 1 metals reacting with chlorine
react vigorously when heated in chlorine gas
- reactivity increases as you go down group
describe group 1 metals reacting with oxygen
- react to form metal oxide e.g - Li20
differences between group 1 metals and transition metals
- more reactive
-they are less dense, strong and harder than transition metals - lower melting points
Group 7s and their colours
- fluorine, reactive, poisonous yellow gas
- chlorine, fairly reactive poisonous dense green gas
- bromine, dense, poisonous, red- brown volatile liquid
-iodine, dark grey crystalline solid or a purple vapour
what do halogens exist as
molecules, pairs of atoms
group 0 elements exist as monoatomic gases, what does this mean?
- they are made up of single atoms not bonded to each other at all
what happens to boiling points ad you go down group 0
they increase as relative atomic masses increase
properties of group 1 metals
- soft
- all have one electron on outer shell
- lower melting and boiling points than other metals
- low densities
