Chem quiz ch.3 and 4

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Last updated 9:37 PM on 10/15/26
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54 Terms

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Hydroxide

OH-

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Hydronium

H3O+

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Ammonium

NH4+

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Nitrate

NO3-

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Sulfate

SO4²-

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Cyanide

CN-

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Phosphate

PO4^-3

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Carbonate

CO3^-2

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Bicarbonate

HCO3-

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Acetate

C2H3O2-

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rank IMFs according to increasing strength of attraction

LDF < polar < Ion-ion

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H bonds can form with which atoms

Fluorine, Oxygen, Nitrogen

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1

mono

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2

di

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3

tri

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4

tetra

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5

penta

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hexa

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hepta

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octa

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nona

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deca

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Formal charge formula

Valence e- -(lone pairs + # of bonds)

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Cation

An atom that loses an e- and becomes positively charged

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Anion

An atom that gains an e- and becomes negatively charged

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Ionic bond

When an e- is given away from a metal to nonmetal

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Covalent bond

When e- are shared

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Nonpolar covalent

e- are shared equally

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Polar covalent

e- are shared unequally

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Examples of nonpolar bonds

  • Any molecule made of one element (O2, N2, Cl2) bc the electronegativity is 0

  • Molecules made of only carbon and hydrogen (CH4, C6H12) bc C-H bond has very small electronegativity difference

  • Symmetrical molecules where the central atom is surrounded by the same terminal atoms and has no lone pairs (CO2, BF3, CCl4


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Examples of polar bonds

  • If the central atom is surrounded by different terminal atoms; creates unequal pull on the e- (CH3Cl, HCN)

  • If electronegativity between bonded atoms is greater than 0.4

  • Molecules containing O-H, N-H, or H-F bonds (H2O, NH3, CH3OH)


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Negative charge (-)

Add an e-

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Positive charge (+)

Take away an e-

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Roman numeral 4

IV

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Roman numeral 6

VI

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Roman numeral 9

IX

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Roman numeral 11

XI

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Nitrite

NO2-

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Hypochlorite

ClO-

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Chlorite

ClO2-

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Chlorate

ClO3-

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Perchlorate

ClO4-

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Dihydrogen phosphate

H2PO4-

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Carbonate

CO3²-

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Chromate

CrO4²-

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Dichromate

Cr2O7²-

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Peroxide

O2²-

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Hydrogen phosphate

HPO4²-

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Sulfite

SO3²-

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Thiosulfate

S2O3²-

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-ate

the form with the more oxygen atoms

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-ite

the form with on fear oxygen atoms than the -ate ion

Example (nitrate= NO3- Nitrite= NO2-)

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-hypo

added infront of the -ite name if there are two less oxygens than the -ate name of the ion

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