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14 Cards in this Set
- Front
- Back
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State the meaning of the term electronegativity |
The power of an atom or nucleus to withdraw or attractelectrons OR electron density OR a pair of electrons(towards itself) |
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State the type of bonding in lithium fluoride.Explain why a lot of energy is needed to melt a sample of solid lithium fluoride. |
IonicStrong or many or lots of (electrostatic) attractions(between ions) |
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Explain why the boiling point of X is lower than that of its straight-chain isomer (X has many branches) |
Because molecule is smaller / less polarisable / has lesssurface (area)/ is more spherical / molecules can’t get asclose to one another (to feel the vdW forces) |
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State the type of cracking that produces a high proportion of ethene and propene.Give the two conditions for this cracking process. |
Thermal (cracking)High pressure AND high temperature |
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Give one reason why excess air is used in the Ostwald Process. |
ensure completereaction or combustion |
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Explain why the AsCl4+ ion has a bond angle of 109.5º |
There are 4 bonds or 4 pairs of electrons (around As)(Electron pairs / bonds) repel equally |
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In a mass spectrometer, the relative abundance of each isotope is proportional to thecurrent generated by that isotope at the detector. Explain how this current is generated. |
Electron(s) transferred / flow (at the detector)(From detector / plate) to the (+) ion |
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State the meaning of the term structural isomers. |
(Compounds with the) same molecular formulaBut different structural formula / different displayedformula/different structures / different skeletal formula |
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Identify a catalyst used in a catalytic converter |
Pt / platinumORPd / palladiumORRh / rhodium |
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Explain, in terms of its structure and bonding, why nickel has a high melting point |
Contains positive (metal) ions or protons or nuclei anddelocalised / mobile / free / sea of electronsStrong attraction between them or strong metallic bonds |
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Explain why nickel is ductile (can be stretched into wires). |
Layers or ions can slide over one another |
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Fluorine and iodine are elements in Group 7 of the Periodic Table. 3 (a) Explain why iodine has a higher melting point than fluorine. |
Iodine has more electrons and is bigger (atom or molecule) so bigger surface area and hence Stronger van der Waals forces between molecules |
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Name the type of bond formed when a molecule of BF3 reacts with an F– ion. Explainhow this bond is formed. Type of bond: Explanation: |
Coordinate bond pair of electrons/ both electrons (on Donated from and donated to the BF3 |
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State the trend in first ionisation energies in Group 2 from beryllium to barium.Explain your answer in terms of a suitable model of atomic structure. Trend: Explanation: |
Decreases, Atomic radius increases as as well as electron removed further from nucleus electron in higher energy level and more shells As group is descended so more shielding |
