Level 3 NCEA flsahcards
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| EN is..... | The measure of attraction an atom has for a pair of bonding electrons
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| IE is... | the minimium energy needed to remove an electron from an atom or ion in the gaseous state
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| AR is... | half the distance between the bonded nuclei
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| EN going across the periodic table... | Increases.
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| EN across the periodic table why... | becasue of the increasing number of protons so there is an increasing attration for electrons
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| IE going across the periodic table... | Increases
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| IE across the periodic table why... | becaue of the increasing attraction for electrons which means more energy is requied to remove them
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| AR going across the periodic table... | Decreases
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| AR across the periodic table why... | increasing attraction for electrons pulls the valance shell closer to the nucleus
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| EN going down the periodic table... | decreases
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| AR going down the periodic table why... | decreasing attraction for electrons so valance shell is further away from nucleus
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| EN going down the periodic table why... | increasing sheilding so there is a decrease in the attraction for electrons
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| IE going down the periodic table... | decreases
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| IE going down the periodic table why... | decreasing attraction for electrons so need less energy to remove them
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| AR going down the periodic table... | increases
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| Cations are what electrons | lost
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| anions are what electrons | gained
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| IR of positive ion | Fewer electrons are attracted more strongly to nucleus so IR is smaller than atom
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| IR of negitive ion | More electrons create more repultion betweeen elctrons so IR is bigger than atom
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| Pure covalent bond EN | 0-0.5
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| Polar covalent bond EN | 0.6-1.5
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| Ionic bond EN | 1.6+
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| Forming anions | electrons are added into orbitals of increasing energy
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| Forming Cations | electrons are removed from 4s before 3d
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| [Ar] | 1s2,2s2,2p6,3s2,3p6
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| Transition metals-Form complex ions | Central metal ion surrounded by ligands. Vacant 3d orbitals on t-metal ions accept these loan bonds
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| Transition metals-Form coloured compounds | Electrons in the incomplete 3d orbital absorb specific wave lengths of light energy. The colour seen is the light energy not absorbed
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| Transition metals-Make good catalysts | Vacant orbitals accept electron pairs from molecules. This strains the bonds in the molecules, encouraging reactions to occur
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| Lower oxidation states are | monatomic ions
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| Higher oxidation states | polyatomic ions
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| T metals lose 4s electrons and then a varying number of unpaired 3d electrons to give varying oxidation states
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| 2 Linear | 2,180, symmetrical
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| Trigonal planar | 3, 120, symmetrical
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| 3 Angular bent | 3, 120, asymmetrical
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| Tetrahedral | 4, 109, symmetrical
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| Trigonal pyramidal | 4, 107, asymmetrical
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| 4 Angular bent | 4,104.5, asymmetrical
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| Linear | 4,109, asymmetrical
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| Trigonal bipyramidal | 5, 90, 120, symmetrical
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| Seesaw | 5, 90, 120, asymmetrical
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| T-shaped | 5, 90, 120, asymmetrical
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| 5 Linear | 5, 90, 120, symmetrical
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| Octahedral | 6, 90, symmetrical
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| Square-based pyramid | 6, 90, asymmetrical
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| Square planar | 6, 90, asymmetrical
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| Polar bond | unequally shared electrons between 2 atoms due to different EN
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| Polar molecule | has an uneven spread of charge
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| Non-polar bond | equally shared electrons between 2 identical atoms due to same EN
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| Non-polar molecule | even spread of charge
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| Intermolecular forces | forces within molecules or between ions
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| Examples of intermolecular forces | covalent bonds, ionic bonds
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| Covalent bonds | a strong attraction between atomic nuclei and shared pair of electrons.
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| Stronger covalent bonds | caused by more electrons being involved
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| Ionic bonding | strong EN attraction between cation and anion
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| Stronger ionic bonds | caused by higher charges
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