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Chem 100 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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
what elements have a variable change?
Any element that can form 2 or more positive ions. | ex: transition elements and group 14,15
26
polyatomic ions
group of covalent bonded atoms that has an overall ionic charge
27
what makes up most of polyatomic ions?
a nonmetal bonded to an oxygen
28
what do polyatomic ions generally end in?
-ate
29
when does a polyatomic ion end in -ite
if it has one less oxygen than -ate
30
which group can form 4 different polyatomic ions with oxygen?
group 7A
31
when do you add the prefix "per-"
when it has one more oxygen than the "ate" form
32
when do you add the prefix "hypo-",
when it has one less oxygen than the "-ite" form
33
List the prefixes and suffixes in order from most oxygen to least.
per- -ate -ate -ite hypo- -ate
34
How do you name polyatomic ions?
positive ion + polyatomic ion
35
Covalent compound
two nonmetals share electrons
36
why can't nonmetals share electrons?
they have high ionization energies
37
covalent bonds
nonmetals share electrons
38
molecule
2 or more atoms that share electrons, AKA covalent bond
39
lewis dot structure/ electron dot formula
shows valence electrons in covalent molecule
40
bonding pair
the electrons that are being shared
41
lone pairs
the electrons that aren't being bonded
42
how are bonding pairs represented on the LDS/EDF?
2 dots or a line
43
Which elements are exceptions to the octet rule? (can form more than 8 electrons?) how many can they form?
P,S,Cl,Br,I | can form 10,12,14 valence electrons
44
double bond
2 pairs of electrons shared
45
triple bond
3 pairs of electrons shared
46
Which elements will not form double or triple bonds?
hydrogen and halogens
47
why do double and triple bonds form?
when there aren't enough valence electrons to complete an octet, so lone pairs are shared
48
resonance structures
all possible ways to write the electron dot formula
49
how do you name covalent bonds?
using full name of first element+ second element's first syllabi+ "-ide"
50
what prefixes can you use in front of elements?
mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
51
electronegativity
ability of atom to attract shared electrons in a bond, it determines if electrons are shared evenly or unevenly
52
which element has the highest electronegativity?
Flourine
53
which generally has a higher electronegativity?
nonmetals
54
transitions have ___ electronegativity
low
55
what is the electronegativity of noble gases?
they dont have any elevtronegativity values
56
nonpolar covalent bond
electrons shared equally, atoms have identical/similiar electronegativity
57
polar covalent bond
electrons arent shared equally because there is an electronegativity difference
58
dipole
polar covalent bond that has a slight charge on each atom
59
if a polar covalent bond has an atom with higher electronegativity the charge is
partially negative
60
if a polar covalent bond has an atom with lower electronegativity the charge is
partially positive
61
what is the acceptable electronegativity difference for a atom to be considered a nonpolar covalent bond?
0.4 or less
62
what is the acceptable electronegativity difference for a atom to be considered a polar covalent bond?
0.5-1.8
63
the polarity of a bond increases as the electronegativity difference____.
increases
64
what is the acceptable electronegativity difference for a atom to be considered an ionic bond?
1.9 or higher
65
valence shell electron pair repulsion(VSEPR) theory?
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
``` linear # of electron groups, bonded atoms and bond angle ```
shape of a molecule, 2 electron groups and 2 bonded atoms | bond angle-180
67
trigonal planar
shape of a molecule, 3 electron groups, 3 bonded atoms, bond angle-120
68
bent
shape of a molecule, 4 or 3 electron groups, 2 bonded atoms | bond angle-120
69
tetrahedral
4 atoms attached to 4 electron groups | bond angle- 109
70
how does a tetrahedral bond?
at the corner of central atoms
71
trigonal pyramidal
4 electron groups, 3 bonds (1 lone pair) | bond angle- 109
72
nonpolar molecules
all bond are nonpolar OR when polar bonds/dipoles cancel each other because of symmetrical arrangement
73
polar molecules
one end of molecule is more negatively charged than another end
74
when does polarity occur
when polar bonds/dipoles dont cancel out
75
when are molecules usually nonpolar?
when a polar molecule with 3 or more atoms contain a lone pair
76
relationship of low attractive force and melting/boiling point
low attractive force= low melting/boiling points
77
relationship of high attractive force and melting/boiling point
high melting and boiling points

Chem 100 (20 decks)

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