Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Cuesta College Chemistry > Chapter 10- Terms > Flashcards

Chapter 10- Terms Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Define lattice energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What makes up a ionic bond?

A

Metal and non metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What type of element makes up a covalent bond?

A

Usually 2 nonmetal bonding also result in sharing of E-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Which bond result in transfer of E-?

A

Ionic bond d

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are metallic bonds?

A

Found in metal to metal bond s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are the characteristics of electron in a ionic bond?

A

Electrons transferred

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the electrons characteristic of a covalent bond?

A

Electrons shared

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are the electron on characteristic of a metallic bond?

A

Electrons are pooled

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is an octet ?

A

Atoms with 8 e-s surround the element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is a duet

A

An element with two e-‘s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Which element is a exception to a stable dueto

A

HE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Which element is a exception to a stable dueto

A

HE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Define bond length

A

Average distance between nuclei

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

When can covalent bonds be stable?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A

It decreases!

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

On the electronegstviity periodic table where do they increase ?

A

To the right and to the top

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the EN for pure covalent?

A

< 0.4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the EN for polar covalent ?

A

0.5-2.0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the EN for ionic bond?

A

2.0 and more

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Which bonding gives you lattice energy?

A

Ionic bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Define a hybrid resonance

A

When a Lewis structure has more than one correct way to draw out a Lewis structure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Is it okay for drawing a Lewis structure with a off amount of electrons.

A

No, take into account the charge in the compound.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What does a student need to do on a quiz or test need to put to show a resonance

A

Put arrow between the two such as
“<—>”

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

How do you show charge when drawing a Lewis structure

A

Put the entire Lewis structure in a brackets and show the charge at the top right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Which bond exerts a greater attraction for the E’s than the other?

A

Polar covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Define electronegativity

A

The ability of an atom in a molecule to attract e-‘s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Define dipole moment

A

Separation of charge

32
Q

Which bond (ionic, polar, metallic ) results in partial charges on atoms?

A

Polar bond

33
Q

How to determine polarity?

A
  1. Identify polar covalent bonds
  2. Determine if polar bonds form a net dipole moment (polar) or cancel one another (non polar)
34
Q

What does formula charge do?

A

Helps find the correct Lewis structure

35
Q

How to find the formal charge?

A
  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
Q

How are molecular shape defined?

A

With angles and distance between the nuclei of adjacent atoms

37
Q

Do chemical properties arise from ∠? Shape, or distance?

A

Shape

38
Q

Define VSEPR Thoery

A

Valence shell e-‘s pair repulsion theory explains the existence of shapes

39
Q

Define e- domain geometry

A

Arrangement of e- domains around the central atom

40
Q

What three things can the VSEPR model do!

A
  1. Reduction the Lewis structure
  2. Determine the electron geometry
  3. Predict the molecular geometry from the electron geometry
41
Q

Do lone pairs disrupt shape of molecules?

A

Yes, lone pairs hold greater repulsive forces on adjacent electron domains and compress bond angles

42
Q

Can central atoms from the 3 period have more than an octet?

A

Yes

43
Q

Based on dipole, how do you determine if a molecule is polar or not?

A

If the dipole vector add up = polar
If dipole vector cancel out = non-polar

44
Q

Define the Lewis theory

A

Atoms share electron to form covalent bonds

45
Q

What electron geometry has 3 electron groups?

A

Trigonal planar

46
Q

What electron geometry has 4electron groups

A

Tetrahedral

47
Q

What electron geometry had 5 electron groups?

A

Trigonal bipyramidal

48
Q

What electron geometry has 6 electron groups?

A

Octahedral

49
Q

3 electron groups and 3 bonding groups calls for what molecular geometry ?

A

Trigonal planar

50
Q

3 electron groups with 2 bonding groups calls for what molecular geometry?

A

Bent

51
Q

4 electron groups and 4 bonding groups calls for what molecular geometry

A

Tetrahedral

52
Q

4 electron groups &3 bonding groups calls for what molecular geometry?

A

Trigonal pyramidal

53
Q

4 electrons groups and 2 bonding groups calls for what molecular geometry

A

Bent

54
Q

5 electrons groups and 5 bonding groups calls for what molecular geometry

A

Trigonal bipyramidal

55
Q

5 electrons groups and 4 bonding groups calls for what molecular geometry

A

Seesaw

56
Q

5 electrons groups and 3 bonding groups calls for what molecular geometry

A

T-shaped

57
Q

5 electrons groups and 2 bonding groups calls for what molecular geometry

A

Linear

58
Q

6 electrons groups and 6 bonding groups calls for what molecular geometry

A

Octahedral

59
Q

6 electrons groups and 5 bonding groups calls for what molecular geometry

A

Square pyramidal

60
Q

6electrons groups and 4 bonding groups calls for what molecular geometry

A

Square planar

61
Q

Define QM model /VSEPR

A

Electrons occupy orbitals of certain shapes

62
Q

Define Lewis theory

A

Atoms share electrons to form covalent bonds

63
Q

Define valence bond theory

A

Atomic orbitals share a region of space / overlap to form covalent bonds

64
Q

Describe the bond in H2.

A

1s - 1s bond

65
Q

A linear aggrangement of electron implies what hybridization?

A

SP hybridization

66
Q

A trigo al planar arrangement of electrons calls for what hybridization?

A

SP2 hybridization

67
Q

A tetrahedral arrangement of electrons calls for what hybridization?

A

SP3

68
Q

A arrangement of trigonal byprymidal electrons calls for what hybridization

A

SP3d

69
Q

An arrangement octahedral of electrons calls for what hybridization?

A

Sp3d2

70
Q

Show the hybdrization about B in BF₃

A
  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
Q

How does pressure affect chemistry

A

Constant collisions between gaseous particles and surface around them

72
Q

What is the equation to find pressure?

A

F/ A = P
F : force acting on a given unit
A: area

73
Q

How is atmospheric pressure created?

A

Gravity causes the atmosphere as a whole to press down on the earths surface

74
Q

What is Coulomb’s law?

A

Potential energy of two charge particles is proportional to the product of two charges divided by the distance between them

75
Q

How do core electrons shield outermost elegrons from nuclear charge?

A

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
Q

What’s the conversion from mmHg to atm

A

760 mmHg / 1 atm

Cuesta College Chemistry (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions