Unit 2 Flashcards
(82 cards)
1
Q
How does the size of a cation correspond to neutral atoms
A
- cations are smaller than neutral atoms
- greater zeff
2
Q
How does the size of an anion correspond to neutral atoms
A
-anions are larger than neutral atoms
- smaller zeff so less attractive to nucleus so they can liv further away
3
Q
How can you compare atomic size
A
- more electrons = bigger
- the same number of electrons than look at protons, less protons= bigger
4
Q
When is a bond covalent
A
- when two atoms of similar electronegativity share electrons
- generally 2 nonmetals
- atom is bound to specific atoms
- when bonds are directional
5
Q
When is a bond ionic
A
- when the bond involves a transfer of electrons
-the large difference in electronegativity
-between a metal cation and a non-metal anion
-metals lose electrons
-nonmetals gain electrons - when bonds are nondirectional
- when a 3d lattice is formed
6
Q
How do you name a compound
A
- Swap charges on elements with each other.
- If the charge isn’t obvious put it with roman numerals
- if the charges are equal you don’t need to put them
7
Q
When is a bond polar covalent?
A
- when the bond is a small electronegativity difference
- two nonmetals
-creates two bond dipoles
8
Q
When is a bond non-polar covalent?
A
- no electronegativity difference
- perfectly shared
-between 2 nonmetals or C+H
9
Q
What is charge
A
the number of protons related to the number of electrons
10
Q
How do you tell the oxidation state of monatomic ions?
A
its the same as the charge
11
Q
How does the oxidation state relate to electron density?
A
- Atoms with more positive oxidation states have less electron density
- atoms with more negative oxidation states have a higher electron density
12
Q
How does bond order relate to bond energy and bond length?
A
- the higher the bond order the higher the bond energy and the shorter the length
- the lower the bond order the lower the bond energy and the longer the bond length
13
Q
What is formal charge
A
the overall charge on a compound
14
Q
How do you calculate formal charge
A
formal charge= valence electrons= nonbonding electrons- 1/2bonding electrons
15
Q
What is a resonance structure?
A
an alternative Lewis structure depiction of the same molecule where atom connectivity stays the same.
- the number of electrons is the same but the electrons are distributed differently
- same valence electrons and connectivity
16
Q
Which atom goes in the middle of a Lewis structure?
A
the least electronegative
17
Q
How many bond domains are a lone pair?
A
1 domain
18
Q
How many bond domains are a single bond
A
1 domain
19
Q
How many bond domains are a double bond
A
1 domain
20
Q
What is molecular geometry?
A
describes the shape of atoms in molecules
21
Q
What is electron geometry?
A
shows the shapes of electrons around the molecule
22
Q
What is the bond angle of 2 electron regions
A
180
23
Q
What is the bond angle of 3 electron regions
A
120
24
Q
What is the bond angle of 4 electron regions
A
109.5
25
What is the electron domain geometry on 2 electron regions
linear
26
What is the electron domain geometry on 3 electron regions
trignol planar
27
What is the electron domain geometry on 4 electron regions
tetrahedral
28
What is the molecular geometry on 2 electron regions
no lone pairs on central atom= linear
29
What is the molecular geometry on 3 electron regions
- no lone pairs= trigonal planar
- 1 lone pair = bent
30
What is the molecular geometry on 4 electron regions
- no lone pairs = tetrahedral
- 1 lone pair= trigonal pyramidal
- 2 lone pairs =bent
31
what bonds does a single bond have
-1 sigma
-0 pi
31
what bonds does a double bond have
-1 sigma
-1 pi
32
what bonds does a triple bond have
- 1 sigma
2 pi
33
What is a sigma bond
- formed by the direct end to end orbital overlap
- all orbitals are capable but they mainly occur in hybridized orbitals
- horizontal bonds
34
What is a pi bond
- can only be formed after a sigma bond
- formed by orbital overlap above and below the nuclear axis
- most commonly formed by overlapping p orbitals
- can be formed by d and f orbitals
- vertical
35
What are unhybridized orbital
orbital with no electrons
36
which bonds are unhybridized
pi bonds
37
What is the hybridization theory
- the orbital structure of atoms in a molecule
-tells about the geometry of a molecule and its bonds
- orbitals of an atom are mixed to form new hybridized orbitals that reside on the atom
- example= sp, sp2, sp3
38
What is the molecular order theory?
- describes the electronic structure using quantum theory
- tells about the electromagnetic properties of molecules
- orbitals of 2+ atoms are mixed to form new molecular orbitals which span across the whole molecule
- example: bonding and antibonding orbitals
39
what is the bond order formula
(1/2) (Be- ABE)
40
What are the characteristics of solids?
-rigid
-fixed volume
-fixed shape
41
What are characteristics of liquids?
-not rigid
- fixed volume
- no fixed shape
42
What are the characteristics of gas?
- not rigid
- no fixed volume
- no fixed shape
43
What is Avogadro's law
volume is proportional to the number of moles
- as long as temperature and pressure are constant
44
What is Boyle's law
volume is inversely proportional to the pressure
- as long as time and number of moles are constant
45
What is Charles Law
volume is directly proportional to the temp
- as long as pressure and number of moles is constant
46
What is the molarity formula
number of moles of a gas/ volume
47
what is an intramolecular force?
exists within a singular molecule
- covalent or ionic bonds between molecules
48
what is an intermolecular force?
between 2 or more molecules
-attractive forces that keep molecules together
49
what is a London dispersion force
temporary induced dipole that forms because of molecular movement
50
which molecules have London dispersion forces
all of them
51
Why do dipoles form
because of electronegativity differences
52
What are the requirements of 2 bond dipoles to symmetrically oppose
- must have a 180 angle
53
What are the requirements of 3 bond dipoles to symmetrically oppose
must have a 120 angle
53
What are the requirements of 4 bond dipoles to symmetrically oppose
must have a 109.5 angle
54
What is a dipole dipole interaction
when the electropositive region of one molecule interacts with the electronegative region of another molecule
- requires two polar molecules
55
What is hydrogen bonding
When the electropositive h atom bonds with an electronegative FON molecule
56
Rank the Bond forces from weakest to strongest
1. LD
2. DD
3. HB
4. Covalent bonding
57
What is vapor pressure
the pressure exerted by a gas in equilibruum with a liquid at a specific temperature
58
What is the relationship between inter molecular forces and vapor pressure
the more forces the lower the vapor pressure
59
What is the relationship between inter molecular forces and melting point
the more forced the higher the melting point
60
what does atmospheric pressure have to do with boiling point?
- the lower the pressure the lower the boiling point
- the higher the pressure the higher the boiling point
61
what is melting
solid to liquid
62
what is freezing
liquid to solid
63
what is evaporation
liquid to gas
64
what is condensation
gas to liquid
65
what is deposition
gas to solid
66
what is sublimation
solid to gas
67
where is the normal melting point
on the solid/ liquid line at 1 atm
68
where is the normal boiling point
on the liquid gas line at 1 atm
69
what is a solute
substance being dissolved
70
what is a solvent
substance doing the dissolving
70
what is a solution
homogeneous mix of solutes and solvent
71
how is a solution formed
- solutes must overcome intermolecular forces holding it together
- solvents must overcome intermolecular forces holding them together
- solutes and solvents must form new intermolecular forces together
72
what does 'like dissolves like" mean
non-polar dissolves non-polar
polar dissolves polar
73
What are ion-dipole interactions?
an ion interacting with the electropositive or electronegative region of another molecule
74
what are electrolyte properties
-dissolved forms ions
-allows for electricity conduction
75
what are weak acid properties
-ionize partially
not extensive
76
what are strong acid characteristics
extensive; reaction takes place completely, ionize completely
77
what are strong base characteristics
ionize completely. all hydroxide compounds that dissolve in water are strong bases
78
Arrhenius Acid
substance produces H30+ ions in aqueous solutions
79
Arrhenius Bases
substances that produces OH- ions in aqueous solutions
