Computer Midterm 2 Review Flashcards by Katie Worms

Hg₂²⁺

Mercury(I)

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NH₄⁺

Ammonium

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NO₂^-

Nitrite

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NO₃^-

Nitrate

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SO₃^2-

Sulfite

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SO₄^2-

Sulfate

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HSO₄^-

Hydrogen sulfate (bisulfate)

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OH^-

Hydroxide

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CN^-

Cyanide

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PO₄^3-

Phosphate

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HPO₄^2-

Hydrogen phosphate

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H₂PO₄^-

Dihydrogen Phosphate

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NCS^- or SCN^-

Thiocyante

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CO₃^2-

Carbonate

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HCO₃^-

Hydrogen Carbonate (bicarbonate)

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ClO^-OCl^-

Hypochlorite

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ClO₂^-

Chlorite

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ClO₃^-

Chlorate

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ClO₄^-

Perchlorate

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C₂H₃O₂^-

Acetate

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MnO₄^-

Permanganate

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Cr₂O₇^2-

Dichromate

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CrO₄^2-

Chromate

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O₂^2-

Peroxide

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C₂O₄^2-

Oxalate

S₂O₃^2-

Thiosulfate

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 2 # of lone pair electrons on 'central' atom: 0

Linear Linear 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 3 # of lone pair electrons on 'central' atom: 0

Trigonal Planar Trigonal Planar 120

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 2 # of lone pair electrons on 'central' atom: 1

Trigonal Planar Bent Less than 120

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 4 # of lone pair electrons on 'central' atom: 0

tetrahedral tetrahedral 109.5

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 3 # of lone pair electrons on 'central' atom: 1

Tetrahedral Trigonal Pyramidal Less than 109.5

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 2 # of lone pair electrons on 'central' atom: 2

Tetrahedral Bent less than 109.5

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 5 # of lone pair electrons on 'central' atom: 0

Trigonal Bipyramidal Trigonal Bipyramidal 90, 120, and 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 4 # of lone pair electrons on 'central' atom: 1

Trigonal Bipyramidal Seesaw 90, 120, and 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 3 # of lone pair electrons on 'central' atom: 2

Trigonal Bipyramidal T-shaped 90 and 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 2 # of lone pair electrons on 'central' atom: 3

Trigonal Bipyramidal Linear 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 6 # of lone pair electrons on 'central' atom: 0

Octahedral Octahedral 90 and 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 5 # of lone pair electrons on 'central' atom: 1

Octahedral Square Pyramidal 90 and 180

Electron-pair Geometry Molecular Geometry Bond Angle of bonding groups/domains on 'central' atom: 4 # of lone pair electrons on 'central' atom: 2

Octahedral Square Planar 90 and 180

Define Isoelectric

Same number of electrons

Define nuclear charge

Attractive force between the protons in the nucleus and the electrons in the energy levels.

More protons = (greater/smaller) nuclear charge

greater

Define shielding

When inner (core) electrons shield outer electrons (valence) from the attractive forces of the nucleus.

Less shielding, electrons pulled (towards/away) nucleus, (more/less) stable, (more/less) energy.

towards, more, less

An orbital that penetrates into the region occupied by core electrons is ____ shielded from nuclear charge and therefore has ______ energy.

less, lower

When drawing arrows for dipoles, arrow points towards molecule that is more . . .

electronegative.

Formal Charge =

Valence e^- - lone e^-- (shared e^-/2)

When doing hybridization, use the ____ geometry.

electron-pair geometry

Lattice Energy =

q₁\* q₂ / r² where q is charge of ion r is distance between them

Lattice energy __________ upon ___________ size of ions.

decreases, increasing

Mercury(I)

Hg₂²⁺

Ammonium

NH₄⁺

Nitrite

NO₂^-

Nitrate

NO₃^-

Sulfite

SO₃^2-

Sulfate

SO₄^2-

Hydrogen sulfate (bisulfate)

HSO₄^-

Hydroxide

OH^-

Cyanide

CN^-

Phosphate

PO₄^3-

Hydrogen phosphate

HPO₄^2-

Dihydrogen Phosphate

H₂PO₄^-

Thiocyante

NCS^- or SCN^-

Carbonate

CO₃^2-

Hydrogen Carbonate (bicarbonate)

HCO₃^-

Hypochlorite

ClO^-OCl^-

Chlorite

ClO₂^-

Chlorate

ClO₃^-

Perchlorate

ClO₄^-

Acetate

C₂H₃O₂^-

Permanganate

MnO₄^-

Dichromate

Cr₂O₇^2-

Chromate

CrO₄^2-

Peroxide

O₂^2-

Oxalate

C₂O₄^2-

Thiosulfate

S₂O₃^2-

Copper Electron Configuration

[Ar]4s¹3d¹⁰

Chromium Electron Configuration

[Ar]4s¹3d⁵

Silver Electron Configuration

[Kr]5s¹4d¹⁰

Naming Acids Simple binary acids consists of: prefix: suffix:

Naming Acids Simple binary acids consists of: plain ion attached to hydrogen prefix: hydro suffix: ic

Naming Acids Polyatomic ion consists of: prefix: suffix:

prefix: na suffix: ic

Naming Acids Polyatomic Ion with extra oxygen prefix: suffix:

prefix: per suffix: ic

Naming Acids Polyatomic Ion one less oxygen prefix: suffix:

prefix: na suffix: ous

Naming Acids Polyatomic Ion with two less oxygen prefix: suffix:

prefix: hypo suffix: ous