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Chem 100 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

what are the most prevalent type of elements in nature?

A

compound

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2
Q

why are noble gases usually found by itself in nature?

A

they are stable because they have an octet

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3
Q

octet rule

A

tendency for atoms to share/transfer electrons to obtain 8 valence electrons

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4
Q

what type of elements are an exception to the octet rule?

A

transition elements

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5
Q

ions

A

electrical charge from gain/loss of electrons

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6
Q

what charge do metals have and why?

A

positive, they have low ionization energies (lose electrons easily)

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7
Q

ionic charge

A

difference between number of protons and number of electrons on upper right hand corner of symbol

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8
Q

cations

A

positively charged ions of metals

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9
Q

why are metal ions smaller than metal atoms?

A

because they lose electrons and its’ energy level decreases

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10
Q

anions

A

negatively charged ions of nonmetals

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11
Q

what ending does anions have?

A

-ide

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12
Q

do nonmetals gain or lose electrons and why?

A

they gain electrons, they have high ionization

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13
Q

What are the charges of elements in group:

1A(1) ,2A(2) ,3A(3) ,7A(17) ,6A(16) ,5A(15)

A 
group 1- 1+
group 2- 2+
group 3- 3+
group 17- 1-
group 16- 2-
group 5- 3-
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14
Q

what are the exceptions of the ionic charge and group number pattern?

A

transition elements, and group 4A(14) do not typically form ions (exception Sn, and Pb)

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15
Q

Ionic compounds

A

compound of positive and negative ions held together by ionic bonds (typically metal and nonmetal)

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16
Q

ionic bonds

A

attraction between positively charged metal ions and negatively charged nonmetal ions

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17
Q

are the physical and chemical properties of ionic compounds similar to its original elements?

A

no

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18
Q

ionic compounds generally have ___melting points and are ____ at room temperature

A

high melting points and

solid at room temperature

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19
Q

chemical formula

A

represents symbols and subscripts in the lowest whole number ratio of the atoms or ions

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20
Q

what is the order of writing a chemical formula?

A

cations first, then anions

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21
Q

How do you name an ionic formula?

A

metal ion first then nonmetal ion (space in between both)

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22
Q

why is it hard to determine the charge of transition elements?

A

because they can lose s and d electrons which allows them to form 2 or more positive ions

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23
Q

which group has the same rule as transition elements when it comes to naming them? and what are the exceptions?

A 
Groups 4A (14) and 5A (15)
exceptions: Zn2+, Ag+, Cd2+
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24
Q

how do you name transition elements?

A

you use roman numerals that represents its ionic charge in parentheses after the cations

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25
Q

what elements have a variable change?

A

Any element that can form 2 or more positive ions.

ex: transition elements and group 14,15

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26
Q

polyatomic ions

A

group of covalent bonded atoms that has an overall ionic charge

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27
Q

what makes up most of polyatomic ions?

A

a nonmetal bonded to an oxygen

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28
Q

what do polyatomic ions generally end in?

A

-ate

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29
Q

when does a polyatomic ion end in -ite

A

if it has one less oxygen than -ate

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30
Q

which group can form 4 different polyatomic ions with oxygen?

A

group 7A

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31
Q

when do you add the prefix “per-“

A

when it has one more oxygen than the “ate” form

32
Q

when do you add the prefix “hypo-“,

A

when it has one less oxygen than the “-ite” form

33
Q

List the prefixes and suffixes in order from most oxygen to least.

A

per- -ate
-ate
-ite
hypo- -ate

34
Q

How do you name polyatomic ions?

A

positive ion + polyatomic ion

35
Q

Covalent compound

A

two nonmetals share electrons

36
Q

why can’t nonmetals share electrons?

A

they have high ionization energies

37
Q

covalent bonds

A

nonmetals share electrons

38
Q

molecule

A

2 or more atoms that share electrons, AKA covalent bond

39
Q

lewis dot structure/ electron dot formula

A

shows valence electrons in covalent molecule

40
Q

bonding pair

A

the electrons that are being shared

41
Q

lone pairs

A

the electrons that aren’t being bonded

42
Q

how are bonding pairs represented on the LDS/EDF?

A

2 dots or a line

43
Q

Which elements are exceptions to the octet rule? (can form more than 8 electrons?) how many can they form?

A

P,S,Cl,Br,I

can form 10,12,14 valence electrons

44
Q

double bond

A

2 pairs of electrons shared

45
Q

triple bond

A

3 pairs of electrons shared

46
Q

Which elements will not form double or triple bonds?

A

hydrogen and halogens

47
Q

why do double and triple bonds form?

A

when there aren’t enough valence electrons to complete an octet, so lone pairs are shared

48
Q

resonance structures

A

all possible ways to write the electron dot formula

49
Q

how do you name covalent bonds?

A

using full name of first element+ second element’s first syllabi+ “-ide”

50
Q

what prefixes can you use in front of elements?

A

mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

51
Q

electronegativity

A

ability of atom to attract shared electrons in a bond, it determines if electrons are shared evenly or unevenly

52
Q

which element has the highest electronegativity?

A

Flourine

53
Q

which generally has a higher electronegativity?

A

nonmetals

54
Q

transitions have ___ electronegativity

A

low

55
Q

what is the electronegativity of noble gases?

A

they dont have any elevtronegativity values

56
Q

nonpolar covalent bond

A

electrons shared equally, atoms have identical/similiar electronegativity

57
Q

polar covalent bond

A

electrons arent shared equally because there is an electronegativity difference

58
Q

dipole

A

polar covalent bond that has a slight charge on each atom

59
Q

if a polar covalent bond has an atom with higher electronegativity the charge is

A

partially negative

60
Q

if a polar covalent bond has an atom with lower electronegativity the charge is

A

partially positive

61
Q

what is the acceptable electronegativity difference for a atom to be considered a nonpolar covalent bond?

A

0.4 or less

62
Q

what is the acceptable electronegativity difference for a atom to be considered a polar covalent bond?

A

0.5-1.8

63
Q

the polarity of a bond increases as the electronegativity difference____.

A

increases

64
Q

what is the acceptable electronegativity difference for a atom to be considered an ionic bond?

A

1.9 or higher

65
Q

valence shell electron pair repulsion(VSEPR) theory?

A

a theory that predicts the shape of a molecule by placing electron pairs on a central atom as far apart as possible to minimize the mutual repulsion of the electrons

66
Q 
linear
# of electron groups, bonded atoms and bond angle
A

shape of a molecule, 2 electron groups and 2 bonded atoms

bond angle-180

67
Q

trigonal planar

A

shape of a molecule, 3 electron groups, 3 bonded atoms, bond angle-120

68
Q

bent

A

shape of a molecule, 4 or 3 electron groups, 2 bonded atoms

bond angle-120

69
Q

tetrahedral

A

4 atoms attached to 4 electron groups

bond angle- 109

70
Q

how does a tetrahedral bond?

A

at the corner of central atoms

71
Q

trigonal pyramidal

A

4 electron groups, 3 bonds (1 lone pair)

bond angle- 109

72
Q

nonpolar molecules

A

all bond are nonpolar OR when polar bonds/dipoles cancel each other because of symmetrical arrangement

73
Q

polar molecules

A

one end of molecule is more negatively charged than another end

74
Q

when does polarity occur

A

when polar bonds/dipoles dont cancel out

75
Q

when are molecules usually nonpolar?

A

when a polar molecule with 3 or more atoms contain a lone pair

76
Q

relationship of low attractive force and melting/boiling point

A

low attractive force= low melting/boiling points

77
Q

relationship of high attractive force and melting/boiling point

A

high melting and boiling points

Chem 100 (20 decks)

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