17779701
Description
Flashcards by Shannon Bradner, updated more than 1 year ago
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Created by Shannon Bradner
about 5 years ago
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| Question | Answer |
| 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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