Chem Exam 1 Memorization

Question 1

Electron configuration for Cr

Answer 1

[Ar} 4s1 3d5

Question 2

Electron configuration for Cu

Answer 2

[Ar] 4s1 3d10

Question 3

Electron configuration for Mo

Answer 3

[Kr] 5s1 4d5

Question 4

Electron configuration for Au

Answer 4

[Xe] 6s¹4f¹⁴5d¹⁰

Question 5

Electron configuration for Ag

Answer 5

[Kr] 4d¹⁰ 5s¹

Question 6

Electronegativity: define and periodic trend

Answer 6

how well an element can attract electrons

increase as you move left to right and up the periodic table (F is most electronegative atom)

–> noble gases are NOT electronegative

Question 7

Ionization Energy (IE): define and periodic trend

Answer 7

Energy required to remove an electron

increases as you move left to right and up the periodic table

–> if equal distance from F, you cannot tell

Question 8

Electron Affinity: define and periodic trend

Answer 8

amount of energy released when electron attaches to neural atom or molecule

increases as you move left to right and up the periodic table

Question 9

Atomic Radius: define and periodic trend

Answer 9

one half the distance between the nuclei

increases right to left and as you go DOWN the periodic table (Fr highest atomic radius)

Question 10

non mental character increases as you…

Answer 10

go left to right and up the periodic table

Question 11

Metallic character increases as you…

Answer 11

go right to left and down the periodic table

Question 12

isoelectronic

Answer 12

same number of electrons=same electron configuration

Question 13

Pauli Exclusion principle

Answer 13

no two electrons in an atom can have the same 4 quantum numbers

Question 14

Aufbau Principle

Answer 14

order in which an atom will fill up its orbitals

Question 15

Principle #

Answer 15

(n) tells you the orbital

Question 16

Angular momentum

Answer 16

(l) tells you shape of orbital

Question 17

m sub l

Answer 17

tells you how many orbitals of each type

Question 18

m sub s

Answer 18

tells you the spin # (either +1/2 or -1/2)

Question 19

Hunds rule

Answer 19

when filling electrons within a subshell, each orbital should be singly occupied with one electron before any orbital is doubly occupied, and all electrons in singly occupied orbitals should have the same spin

Question 20

Ionic Radius

Answer 20

the distance between the nucleus of an ion and the outermost shell of the ion

–> increases as you move down the periodic table

Question 21

Heisenberg uncertainty Model

Answer 21

there is inherent uncertainty in the act of measuring a variable of a particle. Commonly applied to the position and momentum of a particle, the principle states that the more precisely the position is known the more uncertain the momentum is and vice versa

Question 22

Ideal Gas

Answer 22

PV = nRT

Question 23

HON

Answer 23

region of electron density

Question 24

Linear

Question 25

Formal charge

Answer 25

of valence e - # # of lone pairs - # of bonds

Question 26

PO4

Answer 26

phosphate which means ate= ic

Question 27

Ionic compound’s without transition metal

Answer 27

metal + non-mental (make sure to balance charges)

Question 28

Ionic compounds with transition metals

Answer 28

Name of transition metal + roman numeral + metal ending in -ide

Question 29

formal charge

Answer 29

of valence electrons - number of bonds - # of lone pairs

Question 30

Ionic Compound with Polyatomic atom

Answer 30

Name of metal + polyatomic ion

Question 31

Ionic compound transition metal + polyatomic

Question 32

Covalent compound

Answer 32

prefix + name of nonmetal + prefix + nonmetal ending in -ide

Question 33

Acid with oxygen

Answer 33

no prefix, ()ous Acid

Question 34

Acid without oxygen

Answer 34

Hydro (root name)ic Acid

Question 35

J. J. Thompson

Answer 35

Cathode Ray Tube Experiment (discovery of electron) and plum pudding model

Question 36

1 meter

Answer 36

1 x 10^9 nm

Question 37

1 cm

Answer 37

1,000 mm

Question 38

1 meter

Answer 38

100 cm

Question 39

1 kilometer

Answer 39

1,000 meter

Question 40

Hybridization

Answer 40

when HON =

2 –> sp
3 –> sp2
4 –> sp3

HON number is number of bonds around atom (double bonds count as one)

Question 41

sigma bonds

Answer 41

of bonds around atom (double bonds count as 1) - 1

Question 42

pi bonds

Answer 42

2n + n (2n = triple bonds, n = double bonds)

Question 43

when l = 0

Answer 43

s orbital
spherical shape
only one possible drawing

Question 44

when l =1

Answer 44

p orbital
2 lobes
3 possible drawings

Question 45

when l = 2

Answer 45

d orbital
4 leaf clover
5 possible drawings

Question 46

when l = 3

Answer 46

f orbital
tetrahedral (6 lobes)
7 possible orientations