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Cuesta College Chemistry > Chapter 10- Terms > Flashcards

Chapter 10- Terms Flashcards

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1
Q

Define lattice energy

A

Arranged energy from cations and anions to form a crystalline lattice in a ionic solid

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2
Q

What makes up a ionic bond?

A

Metal and non metal

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3
Q

What type of element makes up a covalent bond?

A

Usually 2 nonmetal bonding also result in sharing of E-

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4
Q

Which bond result in transfer of E-?

A

Ionic bond d

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5
Q

What are metallic bonds?

A

Found in metal to metal bond s

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6
Q

What are the characteristics of electron in a ionic bond?

A

Electrons transferred

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7
Q

What are the electrons characteristic of a covalent bond?

A

Electrons shared

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8
Q

What are the electron on characteristic of a metallic bond?

A

Electrons are pooled

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9
Q

What is an octet ?

A

Atoms with 8 e-s surround the element

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10
Q

What is a duet

A

An element with two e-‘s

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11
Q

Which element is a exception to a stable dueto

A

HE

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12
Q

Which element is a exception to a stable dueto

A

HE

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13
Q

Define bond length

A

Average distance between nuclei

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14
Q

When can covalent bonds be stable?

A

In water shared E-‘d create covalent bonds giving stable octects & duets

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15
Q

Is the distance between bonded atoms increased? or decreased? as the # of shared E-‘s increase?

A

It decreases!

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16
Q

What are the quick steps for writing Lewis’s structures for covalent molecules?

A
  1. Write the correct Skeleton for the molecule , most metallic in center & stay symmetrical , hydrogen are always on the end
  2. Find the sum of all E-‘s from elements/atoms
  3. Distribute e-‘s among atoms giving octects
  4. If a atom lacks an octet add a double or triple bond as necessary octects
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17
Q

On the electronegstviity periodic table where do they increase ?

A

To the right and to the top

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18
Q

How to find the electronegatvity difference

A

Subtract the final from the inital electronegativity from the periodic table to find the total (EN ) electronegativity

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19
Q

What is the electric negativity difference for pure covalent, polar covalent & ionic bond?

A

Pure Covalent 0-0.4
Polar covalent 0.4-2.0
Ionic bond 2.0+

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20
Q

What is the EN for pure covalent?

A

< 0.4

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21
Q

What is the EN for polar covalent ?

A

0.5-2.0

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22
Q

What is the EN for ionic bond?

A

2.0 and more

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23
Q

Which bonding gives you lattice energy?

A

Ionic bonding

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24
Q

Can you double count anything that is a bond?
Such as a double bond = how many electron
Triple bond has how many electrons.

A

Yes,
Double bond = 4 electrons
Triple bond = 6 electrons

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25
Define a hybrid resonance
When a Lewis structure has more than one correct way to draw out a Lewis structure.
26
Is it okay for drawing a Lewis structure with a off amount of electrons.
No, take into account the charge in the compound.
27
What does a student need to do on a quiz or test need to put to show a resonance
Put arrow between the two such as “<—>”
28
How do you show charge when drawing a Lewis structure
Put the entire Lewis structure in a brackets and show the charge at the top right
29
Which bond exerts a greater attraction for the E’s than the other?
Polar covalent bond
30
Define electronegativity
The ability of an atom in a molecule to attract e-‘s
31
Define dipole moment
Separation of charge
32
Which bond (ionic, polar, metallic ) results in partial charges on atoms?
Polar bond
33
How to determine polarity?
1. Identify polar covalent bonds 2. Determine if polar bonds form a net dipole moment (polar) or cancel one another (non polar)
34
What does formula charge do?
Helps find the correct Lewis structure
35
How to find the formal charge?
1. Find the electrons for unshared electron & half of the binding electrons are assigned to each atom 2. Subtract assigned electrons from valence electrons for each atom 3. Choose the Lewis structure closely formal charg to zero, all negative charges reside on more EN atoms
36
How are molecular shape defined?
With angles and distance between the nuclei of adjacent atoms
37
Do chemical properties arise from ∠? Shape, or distance?
Shape
38
Define VSEPR Thoery
Valence shell e-‘s pair repulsion theory explains the existence of shapes
39
Define e- domain geometry
Arrangement of e- domains around the central atom
40
What three things can the VSEPR model do!
1. Reduction the Lewis structure 2. Determine the electron geometry 3. Predict the molecular geometry from the electron geometry
41
Do lone pairs disrupt shape of molecules?
Yes, lone pairs hold greater repulsive forces on adjacent electron domains and compress bond angles
42
Can central atoms from the 3 period have more than an octet?
Yes
43
Based on dipole, how do you determine if a molecule is polar or not?
If the dipole vector add up = polar If dipole vector cancel out = non-polar
44
Define the Lewis theory
Atoms share electron to form covalent bonds
45
What electron geometry has 3 electron groups?
Trigonal planar
46
What electron geometry has 4electron groups
Tetrahedral
47
What electron geometry had 5 electron groups?
Trigonal bipyramidal
48
What electron geometry has 6 electron groups?
Octahedral
49
3 electron groups and 3 bonding groups calls for what molecular geometry ?
Trigonal planar
50
3 electron groups with 2 bonding groups calls for what molecular geometry?
Bent
51
4 electron groups and 4 bonding groups calls for what molecular geometry
Tetrahedral
52
4 electron groups &3 bonding groups calls for what molecular geometry?
Trigonal pyramidal
53
4 electrons groups and 2 bonding groups calls for what molecular geometry
Bent
54
5 electrons groups and 5 bonding groups calls for what molecular geometry
Trigonal bipyramidal
55
5 electrons groups and 4 bonding groups calls for what molecular geometry
Seesaw
56
5 electrons groups and 3 bonding groups calls for what molecular geometry
T-shaped
57
5 electrons groups and 2 bonding groups calls for what molecular geometry
Linear
58
6 electrons groups and 6 bonding groups calls for what molecular geometry
Octahedral
59
6 electrons groups and 5 bonding groups calls for what molecular geometry
Square pyramidal
60
6electrons groups and 4 bonding groups calls for what molecular geometry
Square planar
61
Define QM model /VSEPR
Electrons occupy orbitals of certain shapes
62
Define Lewis theory
Atoms share electrons to form covalent bonds
63
Define valence bond theory
Atomic orbitals share a region of space / overlap to form covalent bonds
64
Describe the bond in H2.
1s - 1s bond
65
A linear aggrangement of electron implies what hybridization?
SP hybridization
66
A trigo al planar arrangement of electrons calls for what hybridization?
SP2 hybridization
67
A tetrahedral arrangement of electrons calls for what hybridization?
SP3
68
A arrangement of trigonal byprymidal electrons calls for what hybridization
SP3d
69
An arrangement octahedral of electrons calls for what hybridization?
Sp3d2
70
Show the hybdrization about B in BF₃
1. Find the Lewis structure 2. Count the electron domain around central atom 3. Determine electron geometry (trigonal planar) 4. Determine hybridization from Lewis structure / electron geometry Answer is sp²
71
How does pressure affect chemistry
Constant collisions between gaseous particles and surface around them
72
What is the equation to find pressure?
F/ A = P F : force acting on a given unit A: area
73
How is atmospheric pressure created?
Gravity causes the atmosphere as a whole to press down on the earths surface
74
What is Coulomb’s law?
Potential energy of two charge particles is proportional to the product of two charges divided by the distance between them
75
How do core electrons shield outermost elegrons from nuclear charge?
E- with high probability found closer to the nucleus shield those with high probability of being further away from the nucleus. Outermost electrons are further away from the nucleus and core electrons are closer to the nucleus
76
What’s the conversion from mmHg to atm
760 mmHg / 1 atm

Cuesta College Chemistry (10 decks)

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