Atomic Structure

Question 1

What are the subatomic particles?

Answer 1

Proton- positive charge, 1 amu,
Neutron-no charge, mass around 1 amu
Electron- negative charge and negligible masse

Question 2

What is a nucleus?

Answer 2

The nucleus contains the protons and nuetrons, while electrons move around it.

Question 3

What is atomic number?

Answer 3

The number of protons in a given element

Question 4

Mass number

Answer 4

the sum of an element’s protons and neutrons

Question 5

Atomic mass

Answer 5

essentially equal to the mass number, the sum of an element’s protons and neutrons

Question 6

isotopes

Answer 6

atoms of a given element (same as atomic number) that have different mass numbers. They differ in the number of neutrons

Question 7

What are the three isotopes of hydrogen?

Answer 7

protium, deuterium, and tritium

Question 8

What is atomic weight?

Answer 8

it is the weighted average of the naturally occurring isotopes of and element. The periodic table lists atomic weights, not masses.

Question 9

Who is Rutherford?

Answer 9

first postulated that the atom had a dense, positively charged nucleus that made up only a small fraction of the volume of an atom.

Question 10

What is a Bohr model of an atom?

Answer 10

dense positively charged nucleus is surrounded by electrons revolving around the nucleus in orbits with distinct energy levels.

Question 11

What is a quantum?

Answer 11

The energy difference between energy levels, first described by Planck.

Question 12

What is quantization?

Answer 12

means there is not an infinite range of energy levels available to an electron; electrons can exist only at certain energy levels. The energy of an electron increases the farther it is from the nucleus.

Question 13

What is the atomic absorption spectrum of an element?

Answer 13

it is unique; for an electron to jump from a lower energy level to a higher one, it must absorb an amount of energy precisely equal to the energy difference between the two levels.

Question 14

What is the atomic emission spectrum?

Answer 14

When electrons return from the excited state to the ground state, they emit an amount of energy that is exactly equal to the energy difference between the two levels, and sometimes the electromagnetic energy emitted corresponds to a frequency in visible light range.

Question 15

What is the quantum mechanical model?

Answer 15

it states that electrons do not travel in defined orbits, but rather are localized in orbits; an orbital is a region of space around the nucleus defined by the probability of finding an electron in that region of space.

Question 16

What is the Heisenberg uncertainty principle?

Answer 16

i states that it is impossible to know both an electron’s position and its momentum exactly at the same time.

Question 17

What are the four quantum numbers?

Answer 17

• n, principle
• l, azimuthal
• ml, magnetic
• ms, spin

Question 18

What is the principle quantum number?

Answer 18

n, describes the average energy of a shell

Question 19

What is the azimuthal quantum number?

Answer 19

l, describes the sub-shells within a given principal energy level s, p, d, and f

Question 20

What is the magnetic quantum number?

Answer 20

ml, specifies the particular orbital within a subshell where an electron is likely to be found at a given moment in time.

Question 21

What is the spin quantum number?

Answer 21

indicates the spin orientation (+/- 1/2) of an electron in an orbital.

Question 22

What is the the electron configuration using spectroscopic notation?

Answer 22

(combining the n and l values as a number and letter respectively) to designate the location of electrons. ex the 1s2s2p3s orbitals.

Question 23

what is the n + l rule?

Answer 23

states that the lower of the sum of the vualues of the first and second quantum numbers, n + l, the lower the energy of the subshells. if two subshells possess the same n + l value, the subshell with the lower n value has a lower energy and will fill the electron first.

Question 24

What is Hund’s rule?

Answer 24

a rule that states that sub shell with multiple orbitals (p, d, and f) fill electrons so that every orbital in a sub shell gets one electron before any of them gets a second.

Question 25

Paramagnetic

Answer 25

materials have unpaired electrons that align with magnetic fields, attracting the material to a magnet.

Question 26

Diamagnetic

Answer 26

materials have all paired electrons, which cannot easily be realigned; they are repelled by magnets.

Question 27

What are valence electrons?

Answer 27

electrons that are in the outermost shell, available for interaction (bonding) with other atoms. For groups 1, 2, and 13-18 it is in s and p orbitals. For the transition elements, it is found in the s and either d, or f orbitals

Question 28

What is Avogadro’s number?

Answer 28

NA= 6.02 x 10^23 A mole of things,

Question 29

How is the energy of a quantum determined?

Answer 29

E= hf,

Question 30

What is the angular momentum of an electron proposed by Bohr?

Answer 30

L= nh/2pi, n is the principle quantum number, h is plank’s constant

Question 31

What is plank’c constant

Answer 31

6.626 x 10^-34

Question 32

What is the energy of an electron?

Answer 32

E = -RH/n^2 .

Question 33

What is the Rydberg unit of energy RH?

Answer 33

it is equal to 2.18 x 10 ^18 .

Question 34

What is the ground state?

Answer 34

an atoms lowest energy in which all points are in the lowest possible orbitals.

Question 35

What is the excited state?

Answer 35

It is when at least one electron has moved to a subshell of a higher than normal energy.

Question 36

When electrons go from lower energy to higher energy..

Answer 36

they get AHED .   
A-absorb light
H- higher potential
E- excited 
D- distant .

Question 37

What is a photon?

Answer 37

When an electron is excited to higher level and returns to the ground state, it release energy called a photon

Question 38

How can the electromagnetic energy of a photon be determined?

Answer 38

E=hc/lambda .

Question 39

What is the line spectrum?

Answer 39

where each line on the emission spectrum corresponds to a specific electron transition.

Question 40

What is the Lyman series?

Answer 40

It corresponds to transition energies n is 1 to 2 or more levels.

Question 41

What s the Balmer series?

Answer 41

It is when n=2 and corresponds to transitions energy level 3 or more.

Question 42

What is the Paschen series?

Answer 42

It is when n = 3 and corresponds to transition levels 4 or more.

Question 43

What is E=hc/lambda = -RH[1/ni^2 - 1/nf^2] say?

Answer 43

The energy of emitted photon corresponds to the difference in energy between the higher energy initial state and the lower energy final state.

Question 44

What is the Pauli exclusion principle?

Answer 44

no two electrons in a given atom can possess the same set of four quantum numbers. The position and energy of an electron described by its quantum number is known as its energy state.

Question 45

What is the maximum number within a shell?

Answer 45

2n^2 . n is the principe quantum number.

Question 46

When the difference in energy between 2 shells decreases..?

Answer 46

the distance form the nucleus increases. The energy difference is a function of [1/ni^2 - 1/nf^2] .

Question 47

What is the max number of electrons within a subshell?

Answer 47

4l + 2 .

Question 48

What is the Aufbau principle, or building up principle?

Answer 48

Each subshell will fill completely before electrons begin to enter the next one.

Question 49

What are some notable exceptions to electron configuration?

Answer 49

Chromium and copper, along with other elements in the same group. The electron from the s orbital will move to d, for ex instead of 4s^23d^4 it will be 4s^13d^5. The d filling each orbital outweighs s, but never p.