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Triple Chemistry - Paper C - Flashcards
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- 1During ionic bonding are electrons: Shared? Transferred? Destroyed? Made?Transferred.
- 2Why do atoms create ions?To stabilise themselves / to create a full outer shell.
- 3Do metals gain or lose electrons and what type of ion does it make?They loose electrons creating a positively charged ion (a cation).
- 4If a metal looses 2 electrons what will the resulting charge be?2+
- 5Do non-metals gain or lose electrons and what type of ion does it make?They gain electrons making a negatively charged ion (an anion).
- 6If a non-metal receives 3 electrons, what will the resulting charge be?3-
- 7As you go down groups 1 and 2, do the elements get more or less reactive and why?. More reactive.
. Because the valence electrons are further away from the nucleus meaning they are less attracted and easier to loose. - 8What is the structure of an ionic compound called?A giant regular ionic lattice.
- 9Put in order: Ionic bonds; Intermolecular bonds; Metallic bonds; Covalent bonds. In order of strength from highest to lowest.1. Ionic bonds.
2. Metallic bonds.
3. Covalent bonds.
4. Intermolecular bonds. - 10Explain the conductivity of ionic compounds.. They do not conduct whilst solid as there are no free electrons in the giant regular lattice structure.
. They do conduct when molten or dissolved as the negative ions are free to move around and carry the current. - 11Why do ionic bonds have high melting points?Because the electrostatic / ionic bonds require a lot of energy to break.
- 12List the properties of ionic bonds.. Conductors when dissolved or molten.
. Hard.
. Brittle.
. Form crystals. - 13Describe and explain the structure to metallic bonds have?A regular lattice structure with positive ions and delocalised electrons.
. Positive ions as the metal atoms have lost their valence electrons.
. Delocalised sea of electrons formed by the valence electrons.
.Regular lattice structure formed by the attraction between the positive ions and negative electrons. - 14List the properties of metallic bonding and any potential uses.. High melting and boiling points.
. Malluable.
. React with oxygen to for alkaline metal oxides.
. High tensile strength.
. Strong.
. Used in plating and in electrical wires. - 15How are small molecules made?They are made with covalent bonds between two or more non-metals.
- 16Do small molecules have low or high melting points?Low.
- 17Explain the difference between intermolecular and covalent bonds and what their differences are.. Intermolecular forces are between the separate molecules, holding them together.
. Covalent bonds hold the atoms themsleves together.
. Covalent bonds are strong.
. Intermolecular bonds are weak and very easy to break. - 18List the properties of small molecules.. Low melting and boiling points.
. Non-conductors.
. Gasseous or liquid at room temperature. - 19What is a macromolecule?A giant covalent structure.
- 20List the three main alletropes of carbon.Diamond, graphite and graphene.
- 21What sort of structure does diamond have and how many covalent bonds does it have per carbon atom?. A tetrahedral structure.
. 4 covalent bonds. - 22Explain the properties of diamond.. Tetrahedral structure makes it rigid and lustrous with a high melting and boiling point.
. 4 covalent bonds mean it is a non-conductor and make's it hard. - 23What is the difference between graphite and graphene?Graphene is a single layer of graphite, whereas graphite has many layers of graphene.
- 24What type of structure do most carbon alletropes have that enable it to conduct electricity?A hexagonal structure with three covalent bonds meaning there is one free electrons.
- 25Describe the bonds that are created between sheets of graphene in a graphite structure.They are covalent and extremely weak, allowing the layers to slide over each other.
- 26List some properties of graphene and potential uses.. Transparent.
. Light.
. A good conductor and insulator.
. Useful in pencils and computer microchips. - 27Define an alletrope.A pure element in different physical forms.
- 28Describe the structure of a fullerene, including a description of their properties.. Carbon balls or cylinders that are hollow.
. Arranged in a hexagonal ring structure.
. Very high melting and boiling points, but not as high as graphite and diamond. - 29How big does a particle have to be to be classed as a nanoparticle?Between 1 and 100 nm (nanometres)
- 30Nanoparticles have a high surface area to volume ratio? What does this mean for the nanoparticle?It means a bigger portion of the particle can react on contact.
- 31List some properties of nanoparticles and what they can be used for.. Good catalysts.
. Anti-bacterial and lubricating properties.
. Fullerenes can deliver drugs to the body.
. Good conductors.
. Durable.
. Good for cosmetics like sun cream and deodorants. - 32What are the disadvantages of using nanoparticles?. The effect on the human body isn't fully understood.
. They could be harmful. - 33Describe the structure of a polymer.A long chain of molecules (monomers) with intermolecular bonds.
- 34List the common properties of a polymer.. Weak bonds so the layers can slide over one another.
. Stretched easily.
. Low melting and boiling points.
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- Year 9 Chemistry (Triple Chemistry - Paper C - Bonding, Fullerenes, Alletropes) Karteikarten am Triple Chemistry - Paper C - Flashcards, erstellt von Shannon Bradner am 20/04/2019.
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