Brainscape's Knowledge GenomeTM

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


See full index

CHEM 130 > Quiz 3/Exam 3 - CH 6-8 > Flashcards

Quiz 3/Exam 3 - CH 6-8 Flashcards

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

Electromagnetic radiation

A

A form of energy that travel through space as wav s that move at the speed of light

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

Speed of light

A

3.0 x 10^8 m/s

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

Wavelength, y upside down

A

Distance between two corresponding points on a wave, using meters

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

Frequency, v

A

A measure of the number of wave cycles that move through a point in space in 1 second, units are hertz (Hz)

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

Inversely proportional

A

Wavelength and frequency

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

Frequency and wavelength formula

A

C = yv, c is speed of light

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

Energy of light

A

E photon = hv = hc/y

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

Planck’s constant

A

6.626 x 10^-34 Js

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

Energy of a photon is

A

Directly proportional to the frequency, inversely proportional to the wavelength

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

Orbitals

A

Three-dimensional regions in space where electrons are 95% likely to be found

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

Orbital quantum number (sublevel) l

A

S: spherically shaped, p: dumbbell shaped, d: 4 lobes, f: 8 lobes

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

Aufbau principle

A

Electrons fill orbitals starting with the lowest-energy orbitals

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

Pauli exclusion principle

A

A maximum of two electrons can occupy each orbital and must have opposite spins

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

Hund’s rule

A

Electrons are distributed into orbitals of identical energy (same sublevel) in such a way as to give the maximum number of unpaired electrons

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

Valence electrons

A

Electrons that occupies the valence shell, which is the outer most orbitals in the last-filled (highest n number) principal energy level (S and p for main-group)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Trends in atomic size

A

Decrease from left to right, increase from top to bottom

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

Ionization energy

A

Increased from left to right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Cations are smaller than

A

Their neutral atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

More protons

A

Smaller nucleus

20
Q

Radius

A

Increases top to bottom, decreases left to right

21
Q

Ionization/energy

A

Increases left to right, decreases top to bottom

22
Q

Electronegativity

A

Ability to attract electrons from other atoms (nucleus)

23
Q

Electronegativity activity

A

Decreases left to right, decreases top to bottom, does not apply to noble gases

24
Q

Highest electronegativity

A

Fluorine

25
Q

Lowest electronegativity

A

Frantium

26
Q

Chemical bond

A

A force that holds atoms together in a molecule or compound

27
Q

Ionic bond

A

Cation and anion, electrostatic between oppositely charged ions, transfer of electrons between cation (metal) and anion (nonmetal)

28
Q

Covalent bonds

A

Bond between nonmetals by sharing of electrons between atoms

29
Q

Non polar covalent

A

Equal electron sharing

30
Q

Polar covalent

A

Unequal electron sharing, the one with higher electronegativity will pull electrons towards it

31
Q

The greater the difference in electronegativity

A

The greater the ionic character and

32
Q

Aufbau’s principle

A

Electrons fill orbitals starting with the lowest-energy orbitals

33
Q

Pauli exclusion principle

A

A maximum of two electrons cna occupy each orbital and must have opposite spins

34
Q

Hund’s rule

A

Electrons are distributed into orbitals of identical energy (same sublevel) in such a way as to give the maximum number of unpaired electrons

35
Q

Ionic bond

A

Between oppositely charged ions, cation and anion (metal and nonmetal), extremely strong

36
Q

Covalent bond

A

Nonmetal and nonmetal

37
Q

Non polar covalent bond

A

Equal electron sharing, typically longer bonds, weaker, no difference in electronegativity

38
Q

Polar covalent bonds

A

Unequal electron sharing, typically shorter bonds, stronger

39
Q

The greater the difference in electronegativity

A

The greater the ionic character and the more polar the bond that joins the atoms

40
Q

Covalent bonding: Lewis structures

A
  1. Count total valence electrons 2. Use 6N + 2 to determine the number of bonds (N is number of non-hydrogen atoms) if 6N + 2= VE, single bonds, if = VE + 2, 1 DB, if = VE + 4, either 2 DB or 1 TB
41
Q

Resonance

A

When a molecule can have more than one Lewis structure while only moving electrons (when the structure can be written in more than one way)

42
Q

Parent structures and angles

A

2 pairs = linear and 180°, 3 pairs = trigonal planar and 120°, 4 pairs = tetrahedral and 109.5°

43
Q

Molecular shapes from parent structures : trigonal planar

A

Trigonal planar = 3 bonded, 0 unbonded, bent = 2 bonded, 1 unbonded

44
Q

Molecular shape from parent structure : tetrahedral

A

Tetrahedral = 4 bonded, 0 unbonded, trigonal pyramidal = 3 bonded, 1 unbonded, bent = 2 bonded, 2 unbonded

45
Q

How to determine a molecule is polar

A

Have lone pairs or outside atoms are not the same

CHEM 130 (16 decks)

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