6.2 Electronegativity and polarity

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18 Terms

1
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define electronegativity

the attraction of a bonded atom for the pair of electrons in a covalent bond

2
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why does the electronegativity of bonded atoms of different elements change

1) nuclear charges are different. 2) the atoms may be different sizes. 3) the shared pair of electrons may be closer to one nucleus than the other

3
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describe the Pauling scale

used to compare the electronegativity of atoms of different elements

4
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what charge does an atom with larger electronegativity have

partially negative

5
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what charge does an atom with smaller electronegativity have

partially positive

6
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the bond type if the electronegativity is 0

covalent

7
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the bond type if the electronegativity is 0-1.8

polar covalent

8
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the bond type if the electronegativity is over 1.8

ionic

9
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what type of elements have the most electronegative atoms

the non metals N, O, F, Cl

10
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what type of elements have the least electronegative atoms

the group 1 metals Li, Na, K

11
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define non-polar bond

where the bonded electron pair is shared equally between the bonded atoms

12
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define pure covalent bond

the bonded atoms come from the same element and the electron pair is shared equally

13
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define polar bond

the bonded electron pair is shared unequally between the bonded atoms

14
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define dipole

the separation of opposite charges

15
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define permanent dipole

a dipole in a covalent bond which does not change

16
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explain why CO2 is non-polar

1) each C=O bond has a permanent dipole. 2) the 2 dipoles act in opposite directions and exactly oppose each other. 3) overall the dipoles cancel out. 4) the overall dipole is 0

17
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explain why H2O is polar

1) each O-H bond has a permanent dipole. 2) the 2 dipoles act in different directions but do not oppose each other. 3) overall O is partially negative, H is partially positive

18
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explain how NaCl dissolves in water

1) water molecules attract sodium ions and chloride ions. 2) the ionic lattice breaks down as it dissolves. 3) water molecules surround the sodium ions and chloride ions. 4) sodium ions are attracted toward the oxygen atoms and chloride ions are attracted towards the hydrogen atoms