chapter 5 and 6 chemistry

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what is ionic bonding
the electrostatic attraction between positive and negative ions, holding cations and anions together in ionic compounds.
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ionic bonding properties
giant ionic lattice, conduct electricity as liquids but not solids, solid at room temperature, dissolve in polar solvents
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what are cations and anions
cations are positive, anions are negative
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what is covalent bonding
the electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms, formed in a P orbital overlap.
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what is a dative covalent bond
a covalent bond in which the shared pair of electrons is supplied by only one of the bonded atoms.
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what is electronegativity
the attraction of a bonded atom for the pair of electrons in a covalent bond.
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pauling's scale
across the periodic table, nuclear charge increases, atomic radius decreases, therefore, electronegativity increases.
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electron pair repulsion theory
electron pairs surrounding a central atom determine the shape of the molecule/ion and repel as far away from eachother as possible, changing the angles by 2.5 when there is a lone pair
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shapes of molecules
linear-2 bp=180//trigonal planar,3bp=120,//tetrahedral,4bp=109.5, so 3bp and 1 lp=107,pyrimidal and 2lp and 2bp=non-linear,104.5,
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shapes of molecules 2
trigonal bipyramid,5bp, 120, 90//octahedral,6bp=90
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equation showing electron repulsion trend
bonded pair to bonded pair < bonded pair to lone pair< lone pair to lone pair, so repulsion increases.
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what are the blocks
the 1st 2 groups are the s block, the last 6 groups are the p block, the transition metals are the d block, the lanthanides and actinides are the f block
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s orbital
spherical, start from principal leval 1, with 1 s orbital, increase level, increases radius of s
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p orbital
dumbbell, from level 2 contain 3 p orbitals
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d orbital
various shapes, from level 3, 5 d orbitals
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f orbital
various shapes, from level 4, 7 f orbitals
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london forces
in all molecules, movement of e- produces a changing dipole and at any instant, produces an instantaneous dipole, which induces a dipole on a neighbouring molecule, more e-, more instanteneous dipoles, more induced dipoles, more attractive forces,
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permanent dipole dipole interactions
between permanent dipoles in different polar molecules
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hydrogen bonding
electronegative atoms with one pair of e-, only on oxygen,nitrogen and fluorine, solid ice is less dense than liquid water.
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Other cards in this set

Card 2

Front

ionic bonding properties

Back

giant ionic lattice, conduct electricity as liquids but not solids, solid at room temperature, dissolve in polar solvents

Card 3

Front

what are cations and anions

Back

Preview of the front of card 3

Card 4

Front

what is covalent bonding

Back

Preview of the front of card 4

Card 5

Front

what is a dative covalent bond

Back

Preview of the front of card 5
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