AQA A Level Chemistry
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| What type of bonding exists between metals and non-metals | Ionic bonding
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| What happens to electrons in ionic bonding | They are transferred from metal to non-metal
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| Describe the nature of an ionic bond | The electrostatic attraction between oppositely charged ions
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| Describe the structure of ionic compounds | Giant ionic lattice of positive and negative ions held together by electrostatic forces
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| Explain the melting point of ionic compounds | High melting point because strong electrostatic forces within ionic lattice which require a great deal of energy to break
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| Explain the electrical conductivity of ionic compounds | Conduct when molten or dissolved because ions can move but do not conduct as a solid because ions held in fixed position in lattice
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| Which would you expect to have a higher melting point, NaCl or MgO and why | MgO because ions are double the charge of NaCl so stronger electrostatic forces
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| What is the formula of the ionic compound Aluminium Sulfate | Al2(SO4)3
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| What happens to electrons in covalent bonding | Electrons are shared between non-metal atoms
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| What is the difference between a single and double covalent bond | Single is 2 shared electrons in bond, double is 4 shared electrons
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| Describe the bonding in diamond | Each carbon is bonded to 4 other carbons in a tetrahedral shape
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| Describe the structure of graphite | Layers of carbon atoms arranged in hexagonal pattern with weak bonds and delocalised electrons between layers
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| Explain why graphite conducts electricity | Delocalised electrons are free to move and carry charge
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| Explain the hardness of diamond | Atoms are held in fixed positions
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| What is a co-ordinate (dative) bond | Where one atom contributes both electrons in a covalent bond
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| Give an example of a molecule with co-ordinate bonding | NH4+, AlCl3NH3, CO
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| Why do molecules have different shapes? | Electron pairs repel each other as far apart as possible.
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| Which has the greater repulsion effect lone pair of electrons or a covalent bond? | Lone pair
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| What is the bond angle in a linear molecule? | 180°
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| What is the bond angle in a trigonal planer molecule? | 120°
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| What is the bond angle in a tetrahedral molecule ? | 109°
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| What shape molecule has 6 bonding electron pairs eg SF6, and what is the bond angle | Octahedral, 90 degrees
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| What shape molecule has 5 bonding pairs eg. PCl5 and what are the bond angles | Trigonal bipyramidal, 90 degrees and 120 degrees
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| What is the shape and bond angle of CH4. Why | Tetrahedral, 109.5 degree, electron pairs repel each other as far as possible
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| How do lone pairs affect bond angles | Reduce bonding pair bond angles (by approx. 2 degrees per lone pair) as they repel more than bonding pairs
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| What is the shape and bond angle in water. Why | Bent, 104.5 degree, 4 pairs of electrons including 2 lone pairs
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| What is the shape and bond angle in ammonia. Why | Trigonal Pyramidal, 107. degree, 4 pairs of electrons including 1 lone pair
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| What is the shape and bond angle in SiCl62- Why | Octahedral, 90. degree, 6 bonding pairs of electrons 0 lone pairs
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| Why is the is the bond angle in water less than 180°? | Water contains two bonds and two lone pairs. Lone pairs repel further than bonded pairs of electrons.
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| Where in the periodic table are the most electronegative elements | Top right (not including noble gases)
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| Which is the most electronegative element | Fluorine
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| Which of these bonds will have a dipole? H-C or Cl-C | Cl-C
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| What causes molecule to be polar (2 requirements) | significant differences in electronegativity and asymmetrical shape
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| Why is CCl₄ not a polar molecule? | Symmetrical molecule so dipoles cancel out.
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| Define electronegativity | The ability of an atom to attract electron density (the electron pair) in a covalent bond
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| What causes bond polarity | Differences in electronegativity between two atoms bonded together
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| Draw a diagram to show the polarity of water |
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| Name the 3 types of intermolecular force in order from weakest to strongest | Van der Waals, dipole-dipole and hydrogen bonding
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| Which type of intermolecular force exists between diatomic molecules | Van der waals only
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| Which types of intermolecular force exist in carbon dioxide | Dipole dipole forces
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| Explain how Van der Waals forces arise | Temporary dipoles because of movement of electrons which induce temporary dipoles in neighbouring molecules
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| Explain how dipole dipole forces arise | Partial positive charge attracting partial negative charge
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| Explain why the boiling point of alkanes increase with increasing chain length | More Van der Waals forces
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| Describe the structure of iodine | Molecular lattice of I2 molecules held tougher by Van der Waals forces
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| What 3 elements could be bonded to hydrogen to give hydrogen bonding | Oxygen, nitrogen or fluorine
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| What is a hydrogen bond? | an electrostatic attraction between a proton in one molecule and an electronegative atom in the other.
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| Draw a diagram of water molecules and show the hydrogen bonding |
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| How does hydrogen bonding affect boiling point | Increases boiling point
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| Describe the structure of ice | Regular lattice structure of water molecules held together by hydrogen bonding. Less dense than water
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| Describe the strucutre of metals | Giant metallic lattice of positive metal ions surrounded by delocalised electrons
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| Explain why Mg has a higher melting point than Na | Doubly charged metal ion
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| Explain why metals conduct electricity | Delocalised electrons are free to move and carry charge
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| Explain why metals have high melting points | The delocalised electrons are strongly attracted to the positive metal ions (strong metallic bonds) which requires a lot of energy to overcome
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