Chemistry - Ionic, Covalent and Metallic Bonding

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  • Created by: Jasmin3
  • Created on: 09-04-18 20:20
What are ions and how are they made?
Ions are single or grouped atoms which are made when electrons are transferred.
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Why are electrons transferred?
To fill atoms outershells and become more like the noble gases.
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When metals form ions what happenes to the electrons in their outer shell and what is there charge?
They lose electrons from the outer shell and form positive ions.
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When non-metals form ions what happenes to the electrons in their outer shell and what is there charge?
They gain electrons in their outer shell and form negative electrons.
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The number of electrons lost or gained in ionic bonding is the same as what? Give an example.
Number of electrons lost or gained = same as charge of ion. For example 2 lost, charge is 2+. If 3 are gained, charge is 3-.
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Why are Group 1 and 2 elements most likely to form ion?
They are metals so lose electrons to form positive ions (cations).
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Why are Group 6 and 7 elements most likely to form ions?
They are non-metals so gain electrons to form negative ions (anions).
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Elements in the same _____ have the same number of electrons in their _____ shell. So they have to lose or ____ the ____ number of elements for a full outer shell.
1) group 2) outer 3) gain 4) same
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A sodium atom is in Group 1. What happens to it's electrons when it ionically bonds? What about it's charge?
It loses 1 electron to form a sodium ion with a positive charge.
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An oxygen atom is in Group 6. What happens to it's electrons when it ionically bonds? What about it's charge?
It gains 2 ions to form an oxygen ion with a negative charge.
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Explain why simple ions often have noble gas electronic structures.
Noble gases have a full outer shell in their structure. (1) This makes them a stable struture (1).
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What happens when a metal and non-metal react together?
The metal loses electrons to form a positive charge. The non-metal gains these electrons to form a negative charge.
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When a non-metal and metal react, what force is this called?
Electrostatic force of attraction. They are strongly attracted to each other.
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Draw a dot and cross diagram to show how magnesium chloride (MgCl2) would bond.
_____
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Draw a dot and cross diagram to show how sodium oxide (Na2O) would bond.
_____
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What kind of structure does an ionic compound have?
A giant ionic lattice
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In lattice structures, what is the force, and what is the charge?
They have an electrostatic force of attraction between oppositely charged ions in all directions.
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What 2 properties do ionic compounds all have?
High melting points and high boiling points
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When ionic compounds are solid, liquid and gases, do they carry electricity?
Solid: No, ions held in place, solid structure. Liguid and Gas: Yes, ions are free to move meaning they'll carry electricity.
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How do you find the empirical formula of an ionic compound using a dot and cross diagram?
Count how many electrons each element has, switch the numbers around for the two elements.
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What is covalent bonding?
When non-metal atoms bond together by sharing electrons.
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Why are covalent bonds strong?
They have positivley charged nuclei which are attracted to the shared pair of electrons by electrostatic forces.
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Where do atoms share electrons why?
In their outer shell, highest energy level.
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Each single covalent bond provides how many extra electrons? This enables the electrons to do what?
One, it fills up it's outer shell.
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When does covalent bonding occur?
In compunds of non-metals and non-metal elements
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There is a different dot and cross diagram for covalent bonding. What do the dots show?
The electrons which are shared to complete an atom.
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Draw a dot and cross diagram for ammonia (NH3).
______
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What are simple molecular substances?
Made up of molecules containing a few atoms joined by covalent bonds.
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Name 4 of the most common examples of simple molecular substances.
Hydrogen, Oxygen, Methane, Chlorine, Nitrogen, Water and Hydrogen Chloride.
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Intermolecular substances have _____ covalent bonds but the bonds between are very ____.
Strong, Weak
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Name 3 properties of molecular substances.
Low boiling point, Low melting point, don't conduct electricity
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What state of matter are intermolecular forces?
Liquid or gas
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As the mollecules grow bigger in molecular forces, strength of the force _____ so more ____ is needed to break them.
Increases, energy
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Explain why Oxygen is a gas at room temperature.
The intermolecualr forces are weak and break easily.
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What are polyers?
Long chains of small units that have repeating sections.
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How are atoms in a polymer joined?
By strong covalent bonds
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When drawing a polymer, which bit do you draw and what is this called?
You draw the shortest repeating section called the polythene.
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How do you find the molecular formula of a polymer from a drawing?
Write down the usual formual (how many of element there is) and put an "n" outside the bracket.
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The intermolecular forces molecules are _____ than simple covalent bonds meaning _____,_____ is needed to break them.
Larger, more energy.
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Intermolecular forces are _____ than ionic or covalent bonds so they have ___ boiling points.
weaker, lower
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In giant covalent structures, how are the atoms bonded?
By strong covalent bonds
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Name 3 properties of giant covalent structures.
Very high melting point, Very high boiling point, don't conduct electricity (don't have charged particles).
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Describe diamonds covalent structure.
Each carbon atom forms four covalent bonds, very rigid structure, only carbon.
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Describe graphites covalent structure.
Each carbon atom forms 3 covalent bonds to create layers. Each carbon atom has 1 delocalised electron meaning this carries electricity.
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Give 2 properties of diamond in terms of it's covalent structure.
Strong covalent bonds, doesn't conduct electricity because there are no free electrons. High melting point.
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Give 2 properties of graphite in terms of it's covalent structure.
Has weak covalent bonds so it's soft and slippery. High melting point. Conducts electricity and thermal energy in it's delocalised electron.
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What is graphene?
One layer of graphite joined together in hexagons.
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Give 3 properties of graphene.
The covalent bonds make it strong, it's very light and can carry electricity in it's delocalised electron.
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Give 2 points about a metallic elements outer shell.
The electrons are delocalised. They have strong forces of electrostatic attraction- between positive metal ions and the shared negative electrons.
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What kind of structure do metals have?
They have a 'giant structure'. Atoms are held together in a regular structure known as metallic bonding. This is very strong.
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What substances are held together by metallic bonding?
Metallic elements and alloys.
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Give 4 properties of most metals at room temperature.
Very strong, needs lots of energy to break, high melting and boiling point, solid at room temperature.
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Why are metals good conductors of energy and heat?
There delocalised electrons carry current.
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What are alloys? Why are they better than a pure metal?
Alloys are a mixture of two or more metals or a metal and another element. They are stronger and harder than pure metals so better for everyday use.
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Why are alloys harder than pure metals?
The element mixed with the metal has different sized atoms distorting the layers of the metal atom, making it more difficult to slide over each other.
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What 3 things can change how strong the force is on a material?
1) the structure of the substance 2) the temperature 3) the pressure
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Give 3 properties of a 'solid' structure.
1) Has strong forces, close together in a fixed lattice arrangment. 2) Particles don't move, have a defined shape and volume. 3) Particles vibrate the more they are heated can expand slighlty.
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Give 3 properties of a 'liquid' structure.
1) Have weak forces, are free to move but stick together. 2) Have a definate olume but not shape. 3) Particles are constantly moving randomly , the hotter the faster they move, can expand slighlty.
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Give 3 properties of a 'gas' structrure.
1) Forces are very weak, particles are free to flow. 2) Don;t have a defined shape or volume. 3) Particles constantly move randomly, the hotter the faster they move, can expand slightly.
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What are the state symbols?
(s) - solid (l) - liquid (g) - gas (aq) -aqueous
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What are the 4 changes of state?
Melting (solid to liquid) Condensing ( Gas to Liquid) Freezing ( Liquid to Solid) Boiling (Liquid to Gas)
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Describe how a solid 'melts'.
At a certain tempertaure (melting point) the particles have enough energy to break free from positions, becoming a liquid.
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Describe how a liquid 'boils'.
At a certain tempertaure (boiling point) the particles have enough energy to break their bonds, becoming a gas.
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Describe how a liquid 'freezes'.
At melting point, so many bonds form the particles are held in place, meaning it is now a solid.
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Describe how a gas 'condenses'.
At boiling point, so many bonds have formed and stuck together the particles becoming liquid.
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How do you work out the state of matter from it's temperature?
Solid - Below melting point of substance. Liquid - Between melting and boiling point. Gas - Above boiling point.
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What are nanoparticles?
REALLY tiny particles
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What is the nanoparticle equation?
surface area to volume ratio = surface area/volume
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As nanoparticles decrease in size, what happens to their surface area?
It increases
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Nanoparticles have ____ surface area to volume ratio.
High
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Roughly what size are nanoparticles?
Between 1 and 100 nm
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Other cards in this set

Card 2

Front

Why are electrons transferred?

Back

To fill atoms outershells and become more like the noble gases.

Card 3

Front

When metals form ions what happenes to the electrons in their outer shell and what is there charge?

Back

Preview of the front of card 3

Card 4

Front

When non-metals form ions what happenes to the electrons in their outer shell and what is there charge?

Back

Preview of the front of card 4

Card 5

Front

The number of electrons lost or gained in ionic bonding is the same as what? Give an example.

Back

Preview of the front of card 5
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