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November 17-18 Tests > CHIMISTRY (UNIT 6) > Flashcards

CHIMISTRY (UNIT 6) Flashcards

1
Q

Representative particle of an ionic compound-

A

Formula unit

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2
Q

Representative particle of a covalent substance-

A

Molecule

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3
Q

Why do atoms bond with other atoms?

A

Intermolecular forces

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4
Q

Ionic compound forms between-

A

Metal and nonmetal, or polyatomic ion

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5
Q

What range of electronegativity difference is generally associated with-

A

Polar covalent bond .4 -1.7
Non-polar covalent < .4
Ionic bond > 1.7

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6
Q

State the octet rule-

A

Atoms either transfer or share valence electrons until each atom has 8 valence electrons

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7
Q

Which electrons are shown in a Lewis structure?

A

Valence electrons

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8
Q

Ironically bonded substances are often called-

A

Salts

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9
Q

Compare ironically bonded compounds to molecular compounds in terms of boiling point, hardness, and their ability to conduct electrical current when melted or dissolved-

A

Ionic- high melting and boiling points, good conductor

Covalent- low melting and boiling points, poor conductor

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10
Q

Are ionic or molecular substances more likely to be gases at room temperature-

A

Molecular

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11
Q

What bond is formed when electrons are shared-

A

Covalent bond

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12
Q

Molecular polarity is determined by-

A

Lone pairs and the symmetry of the molecule

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13
Q

Every electron needs 8 valence electrons except-

A

H- 2 valence electrons
Be- 4 valence electrons
B- 6 valence electrons

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14
Q

What is the name of the theory that is used to predict the geometry of molecules-

A

Valence shell electron pair repulsion theory

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15
Q

What is the definition of the “valence shell electron pair repulsion theory”

A

Predicts the geometry of the molecule based on bonds and lone pairs

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16
Q

Abbreviation for “valence shell electron pair repulsion theory”

A

VSEPR

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17
Q

Ionic compounds transfer or share electrons for Lewis structures?

A

Transfer

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18
Q

Covalent bonds transfer or share electrons for Lewis structures?

A

Share

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19
Q

How many atoms and lone pairs does linear have-

A

Atoms- 2
Lone pairs- 0

20
Q

How many atoms and lone pairs does bent have-

A

Atoms- 2
Lone pairs- 2 or 1

21
Q

How many atoms and lone pairs does trigonal planar have-

A

Atoms- 3
Lone pairs- 0

22
Q

How many atoms and lone pairs does trigonal pyramidal have-

A

Atoms- 3
Lone pairs- 1

23
Q

How many atoms and lone pairs does tetrahedral have-

A

Atoms- 4
Lone pairs- 0

24
Q

Which shape(s) will always be polar no matter what?

A

Bent and trigonal pyramidal

25
Q

London dispersion forces definition-

A

a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles

26
Q

Dipole-dipole forces definition-

A

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

27
Q

Hydrogen bonding definition-

A

a bond between the hydrogen atom and more electronegative elements like N, O, and F

28
Q

Molecular formula definition-

A

Exact number of each atom, not simplified

Ex- C(2)H(6)

29
Q

Empire formula definition-

A

Simplified to simplest form

Ex- CaCl(2)

30
Q

Ternary salt definition-

A

Contains 3 different elements (m+nm)

31
Q

Binary salt definition-

A

Contains 2 different elements (m+nm)

32
Q

Molecule definition-

A

One or more elements (nm+nm)

33
Q

1 covalent-

A

Mono

34
Q

2 covalent-

A

Di

35
Q

3 covalent-

A

Tri

36
Q

4 covalent-

A

Tentra

37
Q

5 covalent-

A

Penta

38
Q

6 covalent-

A

Hexa

39
Q

7 covalent-

A

Hepta

40
Q

8 covalent-

A

Octa

41
Q

9 covalent-

A

Nona

42
Q

10 covalent-

A

Deca

43
Q

Why is carbon special when drawing a Lewis structure atom-

A

Always in center if there is one of carbon

44
Q

IMF means what-

A

Intermolecular forces

45
Q

What is intramolecular-

A

existing or taking place within a molecule

46
Q

What is intermolecular-

A

existing or taking place between molecules

November 17-18 Tests (4 decks)

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