Exam 2 Stuff

Question 1

What are the possible values of n?

Answer 1

1 to 7

Question 2

What are the possible values of l?

Answer 2

0 to n-1

Question 3

What are the possible values of m_l?

Answer 3

-l to +l

Question 4

What are the possible values of m_s?

Answer 4

-1/2 or +1/2

Question 5

What is a probability distribution map showing where the electron is likely to be found?

Answer 5

orbital

Question 6

Shows the mathematical derivation of energies and orbitals for an electron in an atom

Answer 6

Schrödinger Equation

Question 7

What does the principal quantum number tell you?

Answer 7

What energy level the electron is in (the period on the periodic table)

Question 8

What does the angular momentum quantum number (l) tell you?

Answer 8

the sublevel (s,p,d,f)

Question 9

What does it mean for an electron to be in the excited state?

Answer 9

the atom absorbed a photon and the electron is moved from a lower orbital to higher

Question 10

What is the probability of finding an electron at a node?

Answer 10

ZERO

Question 11

What does the Pauli Exclusion priciple state?

Answer 11

No 2 electrons in an atom can have the same four quantum numbers.

Question 12

What are degenerate orbitals?

Answer 12

orbitals above the principle quantum number

Question 13

Coulomb’s Law states what?

Answer 13

1. like charges repel
2. opposite charges attract
3. magnitude of interaction increases as charges increase

Question 14

What is sheilding?

Answer 14

An electron is attracted by the nucleus but repelled by the other electrons. Other electrons act like a sheild from full nuclear charge.

Question 15

What is an effective nuclear charge (Z_eff)?

Answer 15

the charge experienced by the electron through the sheild

Question 16

What happens during penetration?

Answer 16

and electron gets closer to the nucleus than the 1s orbital and experiences the full charge of the nucleus

Question 17

What is the Aufbau Principle?

Answer 17

Electrons occupy lower energy levels first and only 2 electrons per oribital

Question 18

What is Hund’s rule?

Answer 18

when filling degenerate orbitals, electrons fill them singly first with parallel spins

Question 19

What are valence electrons?

Answer 19

Electrons in the highest principle energy level

Question 20

What are core electrons?

Answer 20

Electrons that aren’t valence electrons

Question 21

As you move down a column on the periodic table, _____ increases.

Answer 21

density

Question 22

Which way do you move to increase Z_eff?

Answer 22

from right to left across a period

Question 23

Which way do you move on the periodic table to get a bigger radius?

Answer 23

down and left

Question 24

What does it mean to be paramagnetic?

Answer 24

the atom has unpaired electrons and can be attracted by a magnet

Question 25

What does it mean to be diamagnetic?

Answer 25

the atoms has no unpaired electrons, so it is not affected by magnets

Question 26

What happens to atomic radii of cations?

Answer 26

they are much smaller than the corresponding neutral atoms

Question 27

What happens to anions' atomic radii?

Answer 27

They are much larger than their corresponding neutral atoms

Question 28

What is ionization energy?

Answer 28

the enery required to remove an electron from the atom or ion in the gaseous state

Question 29

Which way do you move on the periodic table for ionization energy to increase?

Answer 29

right and up

Question 30

What is electron affinity?

Answer 30

the energy change associated with the gaining of an electron by the atom in the gaseous state

Question 31

Which group has the most negative electron affinity?

Answer 31

the halogens

Question 32

Electron affinity for group 1A becomes more positive as you move ___ the column

Answer 32

down

Question 33

Electron affinity generally becomes more negative as we move to the ___ across a period.

Answer 33

right

Question 34

Which group is the exception to the electron affinity trends?

Answer 34

5A

Question 35

Metallic Character increases as you move ____ and \_\_\_\_

Answer 35

down and left

Question 36

What are bonds that form between a metal and a nonmetal called?

Answer 36

Ionic bonds

Question 37

Ionic compounds in the solid state are composed of a \_\_\_?

Answer 37

lattice

Question 38

Bonds between two or more nonmetals are called?

Answer 38

covalent bonds

Question 39

Covalently bonded atoms form \_\_\_\_?

Answer 39

molecules

Question 40

Name the 7 group two metals.

Answer 40

Chromium, Iron, Cobalt, Copper, Tin, Mercury, Lead