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Chemistry 1 PAP > 3rd Six Weeks > Flashcards

3rd Six Weeks Flashcards

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0
Q

How many types of acids are there?

A

2: containing oxygen & not containing oxygen

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1
Q

Why is are Roman numerals used?

A

Some metals can take more than one charge. The Roman numeral always indicates the charge on the metal in that compound. The Roman numeral does not tell you the number of metal atoms present in the compound.

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2
Q

Naming acids w/out oxygen

A 
Ion Name:
•per\_\_\_ate
•\_\_\_ate
•\_\_\_ite
•hypo\_\_\_ite
Acid Name:
•per\_\_\_ic
•\_\_\_ic
•\_\_\_ous
•hypo\_\_\_ous
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3
Q

True or false: Electrons are almost never shared in pairs.

A

False: Electrons are almost always shared in pairs.

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4
Q

Covalent Bond

A

Two or more valence electrons are shared between two atoms

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5
Q

Single Bond

A

When one pair of electrons are shared between two atoms

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6
Q

The nucleus of the one is attracted to the _______ _________ of the other.

A

Valence electrons

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7
Q

Electronegativity

A

Attraction of one atom for the electrons of another atom (fluorine is the biggest); differences: The type of bond is found by determining the difference (subtract) of the electronegativities

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8
Q

Nonpolar covalent bond

A

When electrons are equally shared between two atoms

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9
Q

Polar covalent bond

A

When electrons are unequally shared

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10
Q

Dipole

A

When a bond or molecule has unequal sharing

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11
Q

Drawing Lewis structures for molecules

A
  1. Count up the number of valence electrons for each atom in the molecule
    -can do this easily by using the group number for each atom in the periodic table
    -adjust the valence electrons if you are drawing the structure for an ion
  2. Draw the atoms bonded together
    -usually the central atom is written first in a molecule, or the atoms in the molecule are written in the order in which they are
    -each bond contains two electrons
  3. Fill in the remaining valence electrons to give all atoms an octet of electrons. leaving the central atom for last
    A. If there are not enough electrons to complete all octets, use multiple bonds.
    B. If there are extra electrons, place them around
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12
Q

Exceptions to the Octet Rule

A
  1. Hydrogen and Helium- both can hold only two electrons
  2. Boron- often has only six electrons
  3. Free radicals- compounds with an odd number of electrons
  4. Atoms with “d” subshells- can hold more than eight electrons
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13
Q

True or False: each pair of bond electrons counts for both of the atoms in the bond

A

True

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14
Q

When an ion has a negative charge, what is required?

A

For this type of ion, surround the structure with brackets and write the charge on the ion outside.

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15
Q

What is VSEPR?

A

Valence shell electron pair repulsion (VSEPR) theory is a model used, in chemistry, to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.

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16
Q

Carbonate

A

Percarbonate: CO4(charge of -2)
Carbonate: CO3(charge of -2)
Carbonite: CO2(charge of -2)
Hypocarbonite: CO(charge of -2)

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17
Q

Sulfate

A

Persulfate: SO5 (charge of -2)
Sulfate: SO4 (charge of -2)
Sulfite: SO3 (charge of -2)
Hyposulfite: SO2 (charge of -2)

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18
Q

Phosphate

A

Perphosphate: PO5(charge of -3)
Phosphate: PO4(charge of -3)
Phosphite: PO3(charge of -3)
Hypophosphite: PO2(charge of -3)

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19
Q

Chlorate

A

Perchlorate: ClO4(charge of -1)
Chlorate: ClO3(charge of -1)
Chlorite: ClO2(charge of -1)
Hypochlorite: ClO(charge of -1)

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20
Q

Iodate

A

Periodate: IO4(charge of -1)
Iodate: IO3(charge of -1)
Iodite: IO2(charge of -1)
Hypoiodite: IO(charge of -1)

21
Q

Acetate

A

Peracetate: C2H3O3(charge of -1)
Acetate: C2H3O2(charge of -1)
Acetite: C2H3O(charge of -1)

22
Q

Manganate

A

Permanganate: MnO4(charge of -1)
Manganate: MnO3(charge of -1)
Manganite: MnO2(charge of -1)
Hypomanganite: MnO(charge of -1)

23
Q

Bromate

A

Perbromate: BrO4(charge of -1)
Bromate: BrO3(charge of -1)
Bromite: BrO2(charge of -1)
Hypobromite: BrO(charge of -1)

24
Q

Bicarbonate

A

Perbicarbonate: HCO4(charge of -1)
Bicarbonate: HCO3(charge of -1)
Bicarbonite: HCO2(charge of -1)
Hypobicarbonate: HCO(charge of -1)

25
Q

Oxalate

A

Peroxalate: C2O5(charge of -2)
Oxalate: C2O4(charge of -2)
Oxalite: C2O3(charge of -2)
Hypoxalite: C2O2(charge of -2)

26
Q

Chromate

A

Perchromate: CrO5(charge of -2)
Chromate: CrO4(charge of -2)
Chromite: CrO3(charge of -2)
Hypochromite: CrO2(charge of -2)

27
Q

Nitrate

A

Pernitrate: NO4(charge of -1)
Nitrate: NO3(charge of -1)
Nitrite: NO2(charge of -1)
Hyponitrite: NO(charge of -1)

28
Q

Arsenate

A

Perarsenate: AsO5(charge of -3)
Arsentate: AsO4(charge of -3)
Arsenite: AsO3(charge of -3)
Hypoarsenite: AsO2(charge of -3)

29
Q

Dichromate

A

Perdichromate: Cr2O8(charge of -2)
Dichromate: Cr2O7(charge of -2)
Dichromite: Cr2O6(charge of -2)
Hypodichromite: Cr2O5(charge of -2)

30
Q

Thiosulfate

A

Perthiosulfate: S2O4(charge of -2)
Thiosulfate: S2O3(charge of -2)
Thiosulfite: S2O2(charge of -2)
Hypothiosulfite: S2O(charge of -2)

31
Q

Bisulfate

A

Perbisulfate: HSO5(charge of -1)
Bisulfate: HSO4(charge of -1)
Bisulfite: HSO3(charge of -1)
Hypobiosulfite: HSO2(charge of -1)

32
Q

Sulfuric acid

A

Persulfuric acid: H2SO5
Sulfuric acid: H2SO4
Sulfurous acid: H2SO3
Hyposulfurous acid: H2SO2

33
Q

Other Polyatomic Ions

A 
Ammonium: NH4(charge of +1)
Hydronium: H3O(charge of +1)
Cyanide: CN(charge of -1)
Peroxide: O2(charge of -2)
Mercury (I): Hg2(charge of +2)
Hydroxide: OH(charge of -1)
34
Q

Carbonic acid

A

Percarbonic acid: H2CO4
Carbonic acid: H2CO3
Carbonous acid: H2CO2
Hypocarbonous acid: H2CO

35
Q

Phosphoric acid

A

Perphosphoric acid: H3PO5
Phosphoric acid: H3PO4
Phosphorous acid: H3PO3
Hypophosphorous acid: H3PO2

36
Q

Iodic acid

A

Periodic acid: HIO4
Iodic acid: HIO3
Iodous acid: HIO2
Hypoiodous acid: HIO

37
Q

Chloric acid

A

Perchloric acid: HClO4
Chloric acid: HClO3
Chlorous acid: HClO2
Hypochlorous acid: HClO

38
Q

Acetic acid

A

Peracetic acid: HC2H3O3
Acetic acid: HC2H3O2
Acetous acid: HC2H3O

39
Q

Oxalic acid

A

Peroxalic acid: H2C2O5
Oxalic acid: H2C2O4
Oxalous acid: H2C2O3
Hypoxalous acid: H2C2O2

39
Q

Manganic acid

A

Permanganic acid: HMnO4
Manganic acid: HMnO3
Manganous acid: HMnO2
Hypomanganous acid: HMnO

40
Q

Bromic acid

A

Perbromic acid: HBrO4
Bromic acid: HBrO3
Bromous acid: HBrO2
Hypobromous acid: HBrO

41
Q

Chromic acid

A

Perchromic acid: H2CrO5
Chromic acid: H2CrO4
Chromous acid: H2CrO3
Hypochromous acid: H2CrO2

42
Q

Nitric acid

A

Pernitric acid: HNO4
Nitric acid: HNO3
Nitrous acid: HNO2
Hyponitrous acid: HNO

43
Q

Arsenic acid

A

Perarsenic acid: H3AsO5
Arsenic acid: H3AsO4
Arsenous acid: H3AsO3
Hypoarsenous acid: H3AsO2

44
Q

Dichromic acid

A

Perdichromic acid: H2Cr2O8
Dichromic acid: H2Cr2O7
Dichromous acid: H2Cr2O6
Hypodichromous acid: H2Cr2O5

45
Q

Thiosulfuric acid

A

Perthiosulfuric acid: H2S2O4
Thiosulfuric acid: H2S2O3
Thiosulfurous acid: H2S2O2
Hypothiosulfurous acid: H2S2O

46
Q

Binary Acids

A

-Must contain Hydrogen in the appropriate numbers to balance the negative charge of the anion
-Prefix of hydro-
-Suffix of -ic
-Root word is nonmetal in shortened form
Examples:
•HCl: Hydrochloric acid
•H2S: Hydrosulfuric acid

47
Q

Shapes, sub-shapes, and bond angles

A

Shapes

  • Linear: 180 degrees; 2 sigma bond pairs & 0 lone pairs
  • Trigonal planar: 120 degrees; 3 sigma bond pairs & 0 lone pairs
  • Tetrahedral: 109.5 degrees; 4 sigma bond pairs & 0 lone pairs
  • Trigonal bypyramidal: 90 degrees & 120 degrees; 5 sigma bond pairs
  • Octahedral: 90 degrees; 6 sigma bond pairs & 0 lone pairs

Sub-shapes

  • Bent (under trigonal planar): ~116 degrees; 2 sigma bond pairs & 1 lone pair
  • Trigonal pyramidal (under tetrahedral): ~107 degrees; 3 sigma bond pairs & 1 lone pair
  • Bent (under tetrahedral): ~105 degrees; 2 sigma bond pairs & 2 lone pairs
  • Unsymmetrical tetrahedron (under trigonal bipyramidal): 4 bond pairs & 1 lone pair
  • T-shaped (under trigonal bipyramidal): 3 bond pairs & 2 lone pairs
  • Linear (under trigonal bipyramidal): 2 bond pairs & 3 lone pairs
  • Square pyramidal (under octahedral): 5 bond pairs & 1 lone pair
  • Square planar (under octahedral): 4 bond pairs & 2 lone pairs
48
Q

Binary Ionic Compounds using Transition Metals Rules

A
  • Atoms combine in whole number ratios.

* The total charge on a compound must be zero.

49
Q

How does symmetry play a role in determining polarity?

A

Symmetrical: Nonpolar
Asymmetrical: Polar

Chemistry 1 PAP (6 decks)

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