Triple Chemistry - Paper C - Flashcards

Frage	Antworten
During ionic bonding are electrons: Shared? Transferred? Destroyed? Made?	Transferred.
Why do atoms create ions?	To stabilise themselves / to create a full outer shell.
Do metals gain or lose electrons and what type of ion does it make?	They loose electrons creating a positively charged ion (a cation).
If a metal looses 2 electrons what will the resulting charge be?	2+
Do non-metals gain or lose electrons and what type of ion does it make?	They gain electrons making a negatively charged ion (an anion).
If a non-metal receives 3 electrons, what will the resulting charge be?	3-
As 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.
What is the structure of an ionic compound called?	A giant regular ionic lattice.
Put 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.
Explain 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.
Why do ionic bonds have high melting points?	Because the electrostatic / ionic bonds require a lot of energy to break.
List the properties of ionic bonds.	. Conductors when dissolved or molten. . Hard. . Brittle. . Form crystals.
Describe 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.
List 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.
How are small molecules made?	They are made with covalent bonds between two or more non-metals.
Do small molecules have low or high melting points?	Low.
Explain 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.
List the properties of small molecules.	. Low melting and boiling points. . Non-conductors. . Gasseous or liquid at room temperature.
What is a macromolecule?	A giant covalent structure.
List the three main alletropes of carbon.	Diamond, graphite and graphene.
What sort of structure does diamond have and how many covalent bonds does it have per carbon atom?	. A tetrahedral structure. . 4 covalent bonds.
Explain 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.
What is the difference between graphite and graphene?	Graphene is a single layer of graphite, whereas graphite has many layers of graphene.
What 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.
Describe 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.
List some properties of graphene and potential uses.	. Transparent. . Light. . A good conductor and insulator. . Useful in pencils and computer microchips.
Define an alletrope.	A pure element in different physical forms.
Describe 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.
How big does a particle have to be to be classed as a nanoparticle?	Between 1 and 100 nm (nanometres)
Nanoparticles 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.
List 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.
What are the disadvantages of using nanoparticles?	. The effect on the human body isn't fully understood. . They could be harmful.
Describe the structure of a polymer.	A long chain of molecules (monomers) with intermolecular bonds.
List 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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Triple Chemistry - Paper C - Flashcards

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