Atomic Structure and Periodic Trends

Question 1

proton charge

Answer 1

1+

Question 2

proton mass

Answer 2

1 amu

Question 3

atomic number

Answer 3

• Z
• number of protons
• nuclear charge
• determines the element

Question 4

neutrons charge

Answer 4

0

Question 5

neutrons mass

Answer 5

1 amu

Question 6

mass number

Answer 6

• A
• number of protons and neutrons
• weighted average all of isotopes

Question 7

isotope

Answer 7

• differs in number of neutrons

Question 8

electron charge

Answer 8

-1

Question 9

electron mass

Answer 9

0 amu

Question 10

charge

Answer 10

• number of protons and electrons

Question 11

C>0

Answer 11

cation

Question 12

C=0

Answer 12

atom

Question 13

C<0

Answer 13

anion

Question 14

Bohr model of the atom

Answer 14

• electrons orbit at fixed distances from the nucleus

- distance between orbits decreases with distance from the nucleus

Question 15

quantization of electron energies

Answer 15

• electron energies are quantized are are related to their fixed radius orbits
• energy increases with distance from the nucleus

Question 16

principle quantum number, n

Answer 16

• describes the radial distance of an electron’s orbit from the nucleus.

Question 17

electron transitions excitation

Answer 17

• electrons absorb only specific, allowed quantities of energy
• allowed energies match the energy difference between an electron’s ground state and excited state.
• initial promotion most difficult

Question 18

electronic transitions relaxation

Answer 18

• electrons in an excited state can return to a lower energy orbit, emitting a photon equal in energy to the energy difference between the energy levels.
• electrons can return to the ground state in a single transition, or in multiple transitions.

Question 19

hydrogen absorption spectrum

Answer 19

• dark bands on a light background

Question 20

hydrogen emission spectrum

Answer 20

• bright bands on a dark background

Question 21

lowest to highest energy of waves in electromagnetic spectrum

Answer 21

• radio
• micro
• IR
• ROYGIV
• UV
• Xray
• Gamma

Question 22

energy of a photon

Answer 22

E = hf = (hc)/λ

Question 23

quantum model of the atom

Answer 23

• electrons exist within 3-D orbitals of various sizes and shapes
• electron energies are quantized and are related to their specific orbital
• four quantum numbers fully describe the electronic structure of the quantum model

Question 24

quantization of electron energies

Answer 24

• energy increases with distance from the nucleus

- energy increases with complexity of the orbital shape

Question 25

energy shell and subshell

Answer 25

• each period corresponds to a different energy shell
• each shell is higher energy and larger than the last.
• each block corresponds to a different energy shell
• each subshell is more complex and higher energy than the last.

Question 26

magnetism and spin

Answer 26

• each subshell higher than s has multiple orbital orientations
• each orbital orientation has the same energy
• each orbital can only hold up to 2 electrons
• each electron can be spin up or spin down

Question 27

Aufbau principle

Answer 27

• electron added to orbitals from lowest to highest energy
• valence electrons are in the highest energy shell
• electrons first removed from valence orbitals (outermost) from highest to lowest energy

Question 28

Hund’s rule

Answer 28

• electrons fill degenerate orbitals one per orbital before pairing
• occupy singly before pairing

Question 29

paramagnetic

Answer 29

• at least one electron is unpaired

- attracted to a magnetic field

Question 30

diamagnetic

Answer 30

• all electrons are paired

- doesn’t like magnetic field

Question 31

Pauli principle

Answer 31

• no two electrons may be identical

- this limits the occupancy of an orbital to a maximum of 2 electrons.

Question 32

column 4 and 9 of d-block

Answer 32

• remove the first electron from the highest s subshell first then add to d subshell.
• then remove the rest from the d subshell.

Question 33

excited state of electron configuration

Answer 33

• any number of configurations that have higher energy than the lowest energy electron configuration
• make sure the configuration has the correct total number of electrons
• the electrons can be in ANY orbital as long as that orbital exists.

Question 34

effective nuclear charge (Zeff)

Answer 34

• the nuclear charge experienced by valence electrons
• the pull of protons on valence electrons
• reduced due to shielding
• increases from left to right and from bottom to top on the periodic table. Points to NY

Question 35

atomic radius

Answer 35

• as the force increases, valence electrons are pulled more strongly toward the nucleus, decreasing atomic radius
• increases from right to left and top to bottom on the periodic table. atomically hot in death valley

Question 36

ionic radius

Answer 36

• valence electron repulsion is slightly increased in anions
• valence electron repulsion is slightly decreased in cations.
• ionic radius increases with increasing negative charge

Question 37

shielding

Answer 37

• core electrons shield the valence electrons from the full nuclear charge
• the nuclear charge experienced by a valence electron is Zeff

Question 38

ionization energy

Answer 38

• the minimum amount of energy required to remove the outermost electron from an atom
• increases from left to right and bottom to top
• less energy to pull of an electron as they are further from the nucleus with increasing atomic radius
• hard to do from for nobel gases.

Question 39

electron affinity

Answer 39

• energy change to add an electron to an atom.
• most elements release energy upon the addition of an electron
• the larger the energy change, the more stable the resulting ion
• becomes more negative from left to right and bottom to top

Question 40

multiple ionization

Answer 40

• as the charge on a given ion increases, so too does its ionization energy
• as the extent of ionization increases, valence electron repulsion decreases.
• the second ionization energy is greater than the first.

Question 41

electronegativity

Answer 41

• the ability of an atom to attract electrons to itself in a covalent bond
• increases from left to right and from bottom to top
• F>O>N>C>O>L>Br>I>S>C=H

Question 42

Acidity

Answer 42

• the measure of a compound’s ability to lower the pH of a solution, donate protons or accept electrons
• depends on the relative stability of the acid and its CONJUGATE BASE!
• as the size of the anion increases, its stability increases
• increases from left to right and from top to bottom on the periodic table. Points to Florida where there is a lot of acidic orange juice.

Question 43

d block

Answer 43

• transition metals

Question 44

s and p blocks

Answer 44

• representative elements

Question 45

f block

Answer 45

• rare earth metals