Quiz 3/Exam 3 - CH 6-8

Question 1

Electromagnetic radiation

Answer 1

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

Question 2

Speed of light

Answer 2

3.0 x 10^8 m/s

Question 3

Wavelength, y upside down

Answer 3

Distance between two corresponding points on a wave, using meters

Question 4

Frequency, v

Answer 4

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

Question 5

Inversely proportional

Answer 5

Wavelength and frequency

Question 6

Frequency and wavelength formula

Answer 6

C = yv, c is speed of light

Question 7

Energy of light

Answer 7

E photon = hv = hc/y

Question 8

Planck’s constant

Answer 8

6.626 x 10^-34 Js

Question 9

Energy of a photon is

Answer 9

Directly proportional to the frequency, inversely proportional to the wavelength

Question 10

Orbitals

Answer 10

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

Question 11

Orbital quantum number (sublevel) l

Answer 11

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

Question 12

Aufbau principle

Answer 12

Electrons fill orbitals starting with the lowest-energy orbitals

Question 13

Pauli exclusion principle

Answer 13

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

Question 14

Hund’s rule

Answer 14

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

Question 15

Valence electrons

Answer 15

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)

Question 16

Trends in atomic size

Answer 16

Decrease from left to right, increase from top to bottom

Question 17

Ionization energy

Answer 17

Increased from left to right

Question 18

Cations are smaller than

Answer 18

Their neutral atoms

Question 19

More protons

Answer 19

Smaller nucleus

Question 20

Radius

Answer 20

Increases top to bottom, decreases left to right

Question 21

Ionization/energy

Answer 21

Increases left to right, decreases top to bottom

Question 22

Electronegativity

Answer 22

Ability to attract electrons from other atoms (nucleus)

Question 23

Electronegativity activity

Answer 23

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

Question 24

Highest electronegativity

Answer 24

Fluorine

Question 25

Lowest electronegativity

Answer 25

Frantium

Question 26

Chemical bond

Answer 26

A force that holds atoms together in a molecule or compound

Question 27

Ionic bond

Answer 27

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

Question 28

Covalent bonds

Answer 28

Bond between nonmetals by sharing of electrons between atoms

Question 29

Non polar covalent

Answer 29

Equal electron sharing

Question 30

Polar covalent

Answer 30

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

Question 31

The greater the difference in electronegativity

Answer 31

The greater the ionic character and

Question 32

Aufbau's principle

Answer 32

Electrons fill orbitals starting with the lowest-energy orbitals

Question 33

Pauli exclusion principle

Answer 33

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

Question 34

Hund's rule

Answer 34

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

Question 35

Ionic bond

Answer 35

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

Question 36

Covalent bond

Answer 36

Nonmetal and nonmetal

Question 37

Non polar covalent bond

Answer 37

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

Question 38

Polar covalent bonds

Answer 38

Unequal electron sharing, typically shorter bonds, stronger

Question 39

The greater the difference in electronegativity

Answer 39

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

Question 40

Covalent bonding: Lewis structures

Answer 40

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

Question 41

Resonance

Answer 41

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)

Question 42

Parent structures and angles

Answer 42

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

Question 43

Molecular shapes from parent structures : trigonal planar

Answer 43

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

Question 44

Molecular shape from parent structure : tetrahedral

Answer 44

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

Question 45

How to determine a molecule is polar

Answer 45

Have lone pairs or outside atoms are not the same