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Scott > Lab 3 & 4 Quiz > Flashcards

Lab 3 & 4 Quiz Flashcards

1
Q

What is an ionic compound?

A

Metal(+) and Nonmetal(-)

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2
Q

Whats a molecular/covalent compound?

A

Two nonmetals(-)

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3
Q

How does an elements position on the periodic table determine the magnitude and charge of its monoatomic cation?

A

Group # tells # of VE’s

Metals lose electrons

This gives the magnitude and positive charge

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4
Q

How does the elements position on the periodic table determine the magnitude and charge of the monoatomic anion?

A

Gain e’s to complete octet rule (8VE)

Gives negative charge(-)

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5
Q

Ionic or Molecular:

Sodium Sulfide

A

Ionic

Na+S2- = Na2S

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6
Q

Ionic or Molecular:

Sulfur Dioxide

A

Molecular

SO2

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7
Q

Ionic or Molecular:

Calcium Hydroxide

A

Ionic

Ca2+OH- = Ca(OH)2

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8
Q

Ionic or Molecular:

Nitrogen Dioxide

A

Molecular

NO2

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9
Q

Ionic or Molecular:

Potassium Oxide

A

Ionic

K+ O2- = K2O

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10
Q

Ionic or Molecular:

Carbon Monoxide

A

Molecular

CO

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11
Q

Ionic or Molecular:

Sodium Phosphate

A

Ionic

Na+ PO43- = Na3PO4

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12
Q

Naming Binary Molecular/Covalent Compounds:

1

A

Mono

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13
Q

Naming Binary Molecular/Covalent Compounds:]

2

A

Di

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14
Q

Naming Binary Molecular/Covalent Compounds:

3

A

Tri

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15
Q

Naming Binary Molecular/Covalent Compounds:

4

A

Tetra

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16
Q

Naming Binary Molecular/Covalent Compounds:

5

A

Penta

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17
Q

Naming Binary Molecular/Covalent Compounds:

6

A

Hexa

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18
Q

Naming Binary Molecular/Covalent Compounds:

7

A

Hepta

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19
Q

Naming Binary Molecular/Covalent Compounds:

8

A

Octa

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20
Q

Naming Binary Molecular/Covalent Compounds:

9

A

Nona

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21
Q

Naming Binary Molecular/Covalent Compounds:

10

A

Deca

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22
Q

What type of compounds use prefixes?

ie: Mono, Di, Tri

A

Covalent/Molecular Compounds

23
Q

Naming Binary Molecular/Covalent Compounds:

SO3

A

Sulfur Trioxide

(no charge = no sulfate)

24
Q

Naming Binary Molecular/Covalent Compounds:

P2O5

A

Diphosphorus Pentoxide

25
Q

Naming Binary Molecular/Covalent Compounds:

CS2

A

Carbon Disulfide

26
Q

Naming Binary Ionic Compounds:

K2S

A

Potassium Sulfide

27
Q

How do you name a binary Ionic compound?

A
  1. Name the metal
  2. Name the nonmetal with the -ide at the end
28
Q

How do you name a ternary Ionic compound?

A
  1. name the metal
  2. name the polyatomic ion
29
Q

How do you name a binary molecular compound?

A
  1. Name 1st element with atoms name
  2. Name the second element using the atoms root with the “-ide” ending.

Use the prefixes to indicate #’s of each atom if more than one.

30
Q

Classify the following compounds as ionic or molecular.

  1. CaO
  2. AgCl
  3. SO2
  4. MgSO4
  5. P2O5
A
  1. ionic
  2. Ionic
  3. Molecular
  4. ionic
  5. Molecular
31
Q

Tetrahedral

A

4 single bonds

32
Q

Pyramidal

A

3 single bonds

33
Q

Planar

A

2 single bonds and 1 double bond

34
Q

Bent

A

1 double bond and 1 single bond

OR

2 single bonds

35
Q

Linear

A

2 double bonds

36
Q

What is the geometry around the central atom?

A

Bent

37
Q

What is the geometry around the central atom?

A

Linear

38
Q

The difference in EN that ranges from 0.5 to 1.9 result in ___________.

A

Polar covalent bond

39
Q

What is the geometry around the central atom?

A

Pyramidal

40
Q

What is the geometry around the central atom?

A

Planar

41
Q

What is the geometry around the central atom?

A

Tetrahedral

42
Q

When the differences in EN are less than 0.5, the bond is considered _____________.

A

nonpolar

43
Q

When the bonds EN is greater than 1.9 the bond is _______.

A

ionic

44
Q

What type of bond is formed when a metal bonds with a nonmetal?

A

Ionic bond

45
Q

What type of bond is formed when a nonmetal bonds with a nonmetal?

A

Molecular bond

46
Q

Two atoms share a pair of VE’s.

A

Covalent Bond

47
Q

A covalent bond where bonding electrons are unequally shared.

A

Polar covalent bond

48
Q

1 pair of e’s shared by 2 atoms

A

Single bond

49
Q

2 pairs of e’s shared by 2 atoms

A

Double bond

50
Q

3 pairs of e’s shared by 2 atoms

A

Tripple bond

51
Q

A formula that lists the # of each type of atoms present in a molecule.

A

Molecular formula

52
Q

A formula that shows which atoms are present in a compound and how they are connected.

A

Structural formula

53
Q
A

Scott (26 decks)

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