Chapter 7 Quantam Mechanics

Question 1

What technology comes from quantum mechanics?

Answer 1

Modern technology

Question 2

Quantum mechanics

Answer 2

Behavior of the small. Electrons are small. We use light to work with them.

Question 3

Light

Answer 3

Electromagnetic radiation.

Question 4

Vertical waves

Answer 4

Electric

Question 5

Horizontal waves

Answer 5

Magnetic

Question 6

Amplitude

Answer 6

Height of wave. Intensity of light

Question 7

Wavelength (Lambda)

Answer 7

Distance covered by wave.

Question 8

Frequency (v)

Answer 8

of waves in a period of time. Direct correlation to energy.

Question 9

Hz

Answer 9

v=nu frequency or cycles/second

Question 10

Relationship between amplitude, wavelength, and frequency.

Answer 10

v=c/lambda

Question 11

Describe the characteristics of Microwaves, Radar, and TV/Radio waves

Answer 11

Infrared end of the spectrum. Long wavelength, Low frequency, Low energy

Question 12

Describe the characteristics of Gamma Rays and X-Rays

Answer 12

Ultra-Violet end of the spectrum. Short wavelength, High frequency, High energy.

Question 13

Planck’s Constant

Answer 13

6.63 x 10(-34) J*S

Question 14

C (Speed of Light)

Answer 14

3 x 10(8)

Question 15

v (nu)

Answer 15

Frequency, 1/s, Hz

Question 16

Lambda -\

Answer 16

Wavelength, nm (1nm =10(-9)m)

Question 17

Interference

Answer 17

Interaction between waves

Question 18

Photoelectric Effect

Answer 18

surfaces emit electrons when a light shines on it.

Question 19

Threshold Frequency

Answer 19

minimum amount of energy needed before electrons are emitted

Question 20

equation for Energy of Photons

Answer 20

E(J) = nhv v= c/(lambda-) therefore, E(J)=h*c/(lambda-) (n=number of photons)

Question 21

Constructive Waves

Answer 21

Waves join together to become larger waves

Question 22

Destructive Waves

Answer 22

Waves cancel each other out.

Question 23

Do particles behave live waves or do they go in a straight line?

Answer 23

Particles behave like waves

Question 24

Spectra

Answer 24

Released light energy

Question 25

Emission spectrum

Answer 25

specific pattern of light related to specific metal

Question 26

Bohr's model of H atoms

Answer 26

H releases energy from higher levels to lower levels. The amount of energy released determines the light emitted.

Question 27

de Broglie said,

Answer 27

"Particles have wave-like characteristics." Who said this?

Question 28

de Broglie concluded if particles (electrons) have waves, what else has waves?

Answer 28

Mass has waves, according to whom?

Question 29

The larger the mass, the ? its wavelike characteristics?

Answer 29

smaller

Question 30

Electron diffraction

Answer 30

when passed through slits, electrons create interference like light. (on off pattern)

Question 31

Complementary view of particles

Answer 31

when one observes wave nature, one cannot observe its particles. vice versa.

Question 32

Heisenberg's Uncertainty Principle

Answer 32

Electrons-- 2 personalities, position and speed. If you know more about position, you know less about its speed. vice versa.

Question 33

Schrodinger come up with what in atoms

Answer 33

Orbitals--90% likelihood of where an electron will be.

Question 34

Quantum numbers

Answer 34

Numeric Address for the atom

Question 35

n (quantum numbers)

Answer 35

energy level (layer)

Question 36

l (L) (quantum numbers)

Answer 36

Sublevel s,p,d, or f. n-1 s=0 p=1 d=2 f=3

Question 37

m(sub L) (quantum numbers)

Answer 37

m(sub L) = +-L

Question 38

m(sub s) (quantum numbers)

Answer 38

+-1/2 depending on electron spin

Question 39

Pauli Exclusion Principle

Answer 39

no two electrons in an atom can have the same four quantum numbers

Question 40

Aufbau principle/Building-Up Principle

Answer 40

A scheme to reproduce the electron configurations of the ground states of atoms by successively filling shells with electrons in a specific order (building-up) order.

Question 41

Valence Electron

Answer 41

An electron in an atom outside the noble-gas or pseudo-noble-gas core. Primarily involved in chemical reactions.

Question 42

Hund's rule

Answer 42

the lowest-energy arrangement of electrons in a subshell is obtained by putting electrons into separate orbitals of the subshell with the same spin before pairing electrons.

Question 43

Probability density

Answer 43

Zone where it is more likely to find an electron near the nucleus.

Question 44

Name the S orbital phases

Answer 44

1s, 2s ![]() 349 × 329 - sparknotes.com

Question 45

Name the P orbital phases

Answer 45

p(x), p(y), and p(z) ![]() 2313 × 894 - chemtube3d.com

Question 46

Name the D orbital phases

Answer 46

d(x2-y2), d(xz), d(dz2), d(xy), d(yz)) ![]() 600 × 400 - chemistry.stackexchange.com

Question 47

Mendeleev was whom?

Answer 47

Father of the periodic table Created Periodic law Predicted new elements Same groups had similar properties

Question 48

Periodic law

Answer 48

the elements are arranged by atomic number, their physical and chemical properties vary periodically.

Question 49

Shielding

Answer 49

electrons shielded from nucleus by other electrons despite attraction to nucleus. Atoms sizes shrink (contract) because of magnetic effect.

Question 50

Atomic radius

Answer 50

van der Waals measured radius by element particles barely touching. Covalent radius is measured by element particles pushing against each other.

Question 51

Paramagnetism

Answer 51

Magnetic....unpaired electrons.

Question 52

Diamagnetic

Answer 52

orbitals are full. not magnetic

Question 53

Cations get smaller why?

Answer 53

When an atom loses electrons there is more magnetic pull from the positive nucleus on the negative electrons.

Question 54

Anions get bigger why?

Answer 54

When an atom gains electrons, the magnetic pull of the nucleus is diluted by the addition negative electron force.