The Periodic Table, metals and non-metals Flashcards
In what order is the elements in the periodic table arranged?
by Proton number
What is it meant by periods and groups of the periodic table
The periods are rows and Groups are columns of the periodic table.
Where are transition elements located in the periodic table.
In the middle block.
What can be predicted using an elements position in the periodic table.
Its properties.
In a periodic table,what is the primary classification of the elemnts
metals and non-metals
Where are most metals in the periodic table located?
To the left of the bold zigzagged line.
What are the properties of metals? [7]
- Shiny appearance.
- Solids, except for Mercury.
- High melting points.
- High densities.
- Good conductors of electricity.
- Good conductors of heat.
- Malleable.
[Many of the properties of Metals are due to metallic bonding]
What are the properties of Non-metals?
- Dull appearance.
- Half are solids and half are gases. Bromine is a liquid.
- Low melting points.
- Low densities.
- Poor conductors of electricity.
- Poor conductors of heat
- Brittle.
Why are metals malleable?
Because the layers of atoms can slide over each other
What is an alloy?
is a mixture of a metal and at least one other element.
Why are alloys harder than pure metal?
In alloys, the atoms of different structures disrupts the layered structure of metals, The layers cannot slide over each other and so it is harder.
Describe Brass, in terms of elements mixed together, its properties and its uses.
- Stronger than copper, but still has very good electrical conductivity.
- Used in electrical fittings.
Describe Duralumin, in terms of elements mixed together, its properties and its uses.
- comprised of 96% aluminium, 4% copper and other metals.
- Stronger than aluminium, yet still low density and lightweight.
- used in aircraft manufacture.
Describe stainless steel, in terms of elements mixed together, its properties and its uses.
- Iron with at least 11% chromium and other metals. e.g, nickel.
- corrosion resistant and stronger than iron.
- used in cutlery.
Describe the reaction between metals and and oxygen.
- Metal oxides formed.
- Ionic solids.
- e.g Calcium + Oxygen - > Calcium oxide
Describe the reaction between a metal and an acid.
- Basic salt is formed.
- Hydrogen produced.
- e.g Zinc + Nitric acid - > zinc Nitrate + Hydrogen.
Describe the electrons in outer shells, Ion charge and reactivity of all groups 1-8. Also, distinguish them between metallic and non-metallic.
- Letts revision guide, page 93.
What are group 1 metals known as?
Alkali metals.
What are the physical properties of Group 1 elements?
-soft, compared to other metals.
-Shiny when cut, but dulls as they react with gases in the air
-Low densities; float on water. Densities increase, going down the group.
-Low melting points, compared to other metals (like iron)
e.g. [Fe: 1540 degrees Celsius]
Li : 180
Na : 98
K : 63
Describe the chemical properties of group 1 elements. What is the trend of reactivity.
Very reactive.
Become more reactive, going down the group.
Why are Group 1 elements generally stored under oil?
They react with water and air.
Describe the general reaction of group 1 elements with water.
They float, fizz (effervescence) and move around. The fizzing is due to hydrogen gas being formed.
Describe the reactions, with water of Lithium, sodium, and potassium.
The reactivity increases, going down the group:
- Li : fizzes less vigorously tan sodium or potassium but does not melt.
- Na: produces enough heat to melt and forms a molten ball as it moves around the surface of water.
- K : So exothermic that potassium melts into a molten ball, the hydrogen catches fire and burns with a lilac flame.
Using general trends in group 1, predict the properties of rubidium which is lower down the group in the periodic table.
-soft metal ball that reacts violently with water.
Why,in terms of electrons, do all group 1 elements show similar characteristics when reacting.
Why do they get more reactive down the group?
All have 1 electron in outer shell.
They can easily lose this electron to leave a full outer shell.
As the number of shells increases, there is a greater distance between the positive neutron and electron, means it is further form attraction and the electrons can be easily lost.
Describe transition elements.
a block of metals in the periodic tale between groups I and III, that have similar properties that behave like typical metals.
In comparison with group I metals, describe the physical properties of transition elements.
- Melting point: Transition elements have high and Group 1 has low.
- Density: transition metals have higher than group 1.
In comparison with group I metals, describe the chemical properties of transition elements.
- color of compounds: transition metals have colored compounds while group 1 has white.
- Reaction with water: Transition metals have slow or no reactions, while Group 1 has vigorous reactions.
- Reaction with acids: usually slow of no reactions while group 1 has violent reactions.
Describe two situations, where transition metals are used as catalysts.
- Iron in Haber process.
2. Vanadium oxide in contact processes of production of sulfuric acid.
What is a recurring difference between transition elements.
Their oxidation states.
What is group VII
The Halogens.
Name 3 common halogens.
Chlorine, iodine and bromine.
Describe the trends seen in halogens.
- They become darker down the group.
- The increase in density down the group.
- Reactivity decreases down the group.
Describe the colour and state of Chlorine, Bromine and Iodine.
Chlorine: a pale green gas
Bromine: Red-Brown liquid.
Iodine: Grey-black solid.
What is are displacement reactions?
are reactions where a more reactive element will displace a less reactive one from its compound.
Why are group VII elements so reactive.
- 7 electrons in the outer shell.
- can easily gain one more.
what is group VIII known as?
the noble gases.
Why are they unreactive?
- full outer shells.
- do not lose, gain or share electrons.
- Mono-atomic.
When are noble gases used?
To provide inert atmospheres.
eg. helium in balloons and argon in light bulbs.
What is the reactivity series?
is a list of metals in the order of reactivity, the most reactive, being at the top.
The more reactive a metal is…
- the easier it is to form compounds.
- the harder it is to break its compounds down.
list the reactivity series.
potassium stop calcium magnesium aluminium [carbon] zinc Iron [Hydrogen] copper
For potassium, sodium and calcium, describe its reaction with steam and HCl
- steam: fizz in cold water, giving off hydrogen gas and forming an alkaline hydroxide solution.
- HCl: Violent and explosive.
For Magnesium, zinc and Iron,describe its reaction with steam and HCl.
- Steam: produce hydrogen gas, and metal oxide.
- HCl: produce a salt, giving off hydrogen gas.
For copper, describe its reaction with steam and HCl.
no reactions.
Describe displacement in terms of position in the reactivity series.
Metals higher up, displace metals lower down.
Describe Aluminium’s displacement of Iron from iron(III)oxide.
-Aluminum form ions more easily that iron. so will displace.
-Energy is released- so exothermic, iron melts.
-Oxidation of Al; oxidation sates increasing from 0 to +3
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