Chapter 5: Electrons in Atoms

Question 1

amplitude

Answer 1

the wave’s height from the origin to a crest, or from the origin to a trough

Question 2

atomic emission spectrum

Answer 2

the set of frequencies of the electromagnetic waves emitted by atoms of the element. Each element has its own unique spectrum.

(think of neon signs and how they only come in specific colors.)

Question 3

atomic orbital

Answer 3

a 3-D region around the nucleus. It describes the electron’s probable location.

Question 4

aufbau principle

Answer 4

a

Question 5

de Broglie equation

Answer 5

λ=h/mv
m= particle of mass v= velocity
predicts that all moving particles have wave characteristics

Question 6

electromagnetic radiation

Answer 6

a form of energy that exhibits wavelike behavior as it travels through space. According to Einstein in 1905, is both wavelike & particle like

Question 7

electromagnetic spectrum

Answer 7

aka the EM spectrum. Encompasses all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths.

(short λ bend more than long λ, which results in the Roy. G. Biv sequence)

Question 8

electron configuration

Answer 8

a

Question 9

electron-dot structure

Answer 9

a

Question 10

energy sublevel

Answer 10

labeled s, p, d, f (Smart People Do Fine or Stupid Ppl Do Fail), contained in the principal energy levels. The # of energy sublevels in a principal energy level INCREASES AS n INCREASES.

Question 11

frequency

Answer 11

(represented by v) the number of waves that pass a given point per second.

Question 12

ground state

Answer 12

the lowest allowable energy state of an atom.

When atoms gain energy they are said to be in an excited state.

Question 13

Heisenberg uncertainty principle

Answer 13

states that it is fundamentally impossible to know precisely both the VELOCITY and POSITION of a particle at the same time

Question 14

Hund’s rule

Answer 14

a

Question 15

Pauli’s exclusion principle

Answer 15

a

Question 16

photoelectric effect

Answer 16

electrons (photoelectrons) are emitted from a metal’s surface when light of a certain frequency shines on the surface.
Ex: calculator

Question 17

photon

Answer 17

a particle of electromagnetic radiation with no mass that carries a quantum of energy

photon’s energy:
E = hv
photon

Question 18

Planck’s constant

Answer 18

has a value of 6.626x10^-34 J*s
J= joule (SI unit of energy)
For a given v, matter can emit or absorb energy only in whole-# multiples of hv.

Question 19

principal energy level

Answer 19

n specifies the atom’s major energy levels. (see principal quantum number). An atom’s lowest principal energy level is given a principal quantum # of 1.

Question 20

principal quantum number

Answer 20

(n) indicates the relative sizes and energies of atomic orbitals. As n increases, the orbital becomes larger, the e- spends more time farther from the nucleus, and the atom’s energy level increases.

Question 21

quantum

Answer 21

the minimum amount of every that can be gained or lost by an atom

Question 22

quantum mechanical model of the atom

Answer 22

the atomic model in which electrons are treated as waves (aka the wave mechanical model of the atom) Created by Austrian Erwin Schrodinger, this model makes no attempt to describe the electron’s path around the nucleus.

Question 23

valence electron

Answer 23

a

Question 24

wavelength

Answer 24

(represented by λ) the shortest distance between equivalent points on a continuous wave.
Ex: crest-crest or trough-trough

Question 25

What is the SI unit of frequency

Answer 25

the hertz (Hz). It equals 1 wave/second

Question 26

speed of light

Answer 26

c=λv
ALL electromagnetic waves travel at a speed of 3.00x10^8 m/s in a vacuum. The speed of light is the product of its (λ) and its (v).

Question 27

Max Planck

Answer 27

German physicist who concluded that matter can gain or lose energy only in small, specific amounts called quanta.
E = hv
quantum
where E is energy, h is Planck’s constant and v is frequency

Question 28

quantized

Answer 28

only certain values are allowed

Question 29

Bohr’s model

Answer 29

explained H’s spectral lines, but failed to explain spectrum of any other element. It was also later proved to be fundamentally incorrect. (electrons don’t move around the nucleus in circular orbits)

Question 30

orbitals

Answer 30

s orbitals: spherical
p orbitals: dumbbell shaped
contain no more than 2 electrons

Question 31

Important chem relationship

Answer 31

Atoms in the same group have similar chem properties bc they have the same # of valence electrons