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Chemistry > Unit 10: Covalent Compounds > Flashcards

Unit 10: Covalent Compounds Flashcards

1
Q

When do covalent bonds form?

A

When atoms SHARE ELECTRONS to complete octets.

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2
Q

Covalent bonds form between…

A

two non-metals (groups 4A-7A)

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3
Q

What are used in the names of covalent compounds?

A

prefixes

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4
Q

prefix for 1

A

mono

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5
Q

mono

A

prefix for 1

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6
Q

prefix for 2

A

di

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7
Q

di

A

prefix for 2

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8
Q

prefix for 3

A

tri

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9
Q

tri

A

prefix for 3

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10
Q

prefix for 4

A

tetra

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11
Q

tetra

A

prefix for 4

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12
Q

prefix for 5

A

penta

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13
Q

penta

A

prefix for 5

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14
Q

prefix for 6

A

hexa

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15
Q

hexa

A

prefix for 6

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16
Q

prefix for 7

A

hepta

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17
Q

hepta

A

prefix for 7

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18
Q

prefix for 8

A

octa

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19
Q

octa

A

prefix for 8

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20
Q

prefix for 9

A

nona

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21
Q

nona

A

prefix for 9

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22
Q

prefix for 10

A

deca

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23
Q

deca

A

prefix for 10

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24
Q

How to name covalent compounds:

A

STEP 1 Name the first nonmetal by its element name.
STEP 2 Name the second nonmetal with an ide ending.
STEP 3 Add PREFIXES to indicate the number (from subscripts) of atoms of each nonmetal.

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25
Q

In a hydrogen molecule (H2), each H atom… (3)

A
  1. shares electrons to form a SINGLE COVALENT BOND
  2. acquires TWO electrons.
  3. becomes STABLE like helium (He).
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26
Q

What does a covalent bond indicate?

A

the atoms share electrons

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27
Q

In a fluorine F2 molecule, each F atom…(2)

A
  1. shares ONE electron.
  2. acquires an OCTET (8 electrons)
28
Q

Which orbital does the bonding pair come from? (for molecules that form octets?

29
Q

If carbon has 4 valence electrons, how many bonds can it form?

30
Q

The number of covalent bonds can be determined from…

A

the number of electrons needed to complete an octet

31
Q

Steps to writing electron-dot formulas

A

STEP 1 Determine the arrangement of atoms.
STEP 2 Determine the total number of valence electrons.
STEP 3 Attach each bonded atom to the central atom with a pair of electrons.
STEP 4 Place remaining electrons as lone pairs to complete octets (2 for H atoms).
STEP 5 If octets are not complete, form a multiple bond by converting a lone pair to a bonding pair.

32
Q

How many electrons are shared in a single bond?

33
Q

How many electrons are shared in a double bond?

34
Q

How many electrons are shared in a triple bond?

A

Three Pairs

35
Q

What bond does a nitrogen molecule have?

36
Q

How to count lone pairs?

A

The pairs attached to the central atom that are not in a bond

37
Q

Exceptions to the octet rule

A

group 3 elements, elements on the 3rd row, and beryllium and chloride

38
Q

Why are there exceptions for group 3 elements?

A

they only have 3 valence electrons to bond with

39
Q

Why are there exceptions to elements on the 3rd row?

A

Elements on the 3rd row have the d-orbital available to place surplus electrons

40
Q

Why are there exceptions to beryllium and chloride?

A

has a small atomic radius, which makes it small enough

41
Q

Polar molecules

A

molecules that contain polar bonds

42
Q

Nonpolar molecules

A

molecules that contain no polar bonds or have a symmetrical arrangement of polar bonds

43
Q

Polar bonds

A

Covalent Bonds with an unequal share of electrons because onr end has a higher electron density

44
Q

Nonpolar bonds

A

Covalent bonds with an equal share of electrons

45
Q

Though atoms often form compounds by sharing electrons, the electrons are not always _________

A

SHARED EQUALLY

46
Q

When two atoms share electrons unequally, a ______ results.

47
Q

The greater the difference in electronegativity, the __________ the bond is.

A

More Polar

48
Q

Electronegativity difference for nonpolar

49
Q

Electronegativity difference for polar

50
Q

Electronegativity difference for ionic

51
Q

Are polar molecules symmetrical or asymmetrical?

A

asymmetrical

52
Q

Are nonpolar molecules symmetrical or asymmetrical?

A

symmetrical

53
Q

Polar molecules must contain…

A

polar bonds

54
Q

How can polar bonds be determined?

A

through differences in electronegativity of atoms

55
Q

Symmetrical Molecules have…

A

polar bonds that cancel each other out

56
Q

Examples of symmetrical molecules

A

Linear (more than 2 atoms), Tetrahedral, Trigonal Planar

57
Q

Examples of Asymmetrical molecules

A

Bent and Linear w/ 2 Atoms

58
Q

What forces form between ionic compounds?

A

electrostatic interactions

59
Q

What forces form between covalent compounds?

A

dipole-dipole, hydrogen bonds, (London) dispersion forces

60
Q

Electrostatic interactions are the ______ forces

61
Q

Dispersion forces are the ________ forces

62
Q

Dipole-dipole attractions

A

interaction between +ve end of one molecule and a -ve end of another

63
Q

Hydrogen Bond forms when

A

Hydrogen atoms in one molecule are attracted to the atoms F, O, or N in another molecule.

64
Q

Dispersion forces are…

A

Weak attractions between nonpolar molecules and caused by the MOVEMENT OF ELECTRONS

65
Q

Dipole Moment

A

a measure of the separation of positive and negative charges within a system, or its overall polarity

(magnitude 1 x distance between atoms)

Chemistry (10 decks)

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