chem exam 2 (chapter 3-5)

Question 1

principle quantum number

Answer 1

energy = distance

Question 2

angular quantum number

Answer 2

shape of orbit (which orbital it is)

Question 3

magnetic quantum number

Answer 3

how many of each shape

Question 4

spin quantum number

Answer 4

represents whether an electron is spin up in a magnetic field or spin down

Question 5

Pauli Exclusion Principle

Answer 5

no 2 electrons can have the same 4 quantum numbers

Question 6

paramagnetic

Answer 6

has a magnetic moment

Question 7

diamagnetic

Answer 7

no magnetic moment

Question 8

Hund’s Rue

Answer 8

electrons fill orbitals 1 at a time with parallel spin orbital diagrams

Question 9

Zeff formula (effective nuclear charge)

Answer 9

number of protons - shielding electrons

Question 10

Zeff trend

Answer 10

how strongly the nucleus is holding onto the electrons. Goes up as you go up and to the right

Question 11

Ex: find the Zeff of Na and write the electron configuration

Answer 11

Zeff = # protons - # shielding electrons = 11 - 10 = +1

Electron config: [Ne]3s^1

Question 12

Aufgau Principle

Answer 12

when filling electron shells, fill from the lowest energy level and move up

Question 13

Ionic Bonding

Answer 13

between a metal and a non metal. metal gives electrons to non metal

Question 14

Lewis Dot Models

Answer 14

represent valence electrons on an atom

Question 15

Electronegativity

Answer 15

how tightly an atom hangs onto its valence electrons

Question 16

electronegativity trend

Answer 16

an atom with a smaller radius or more valence electrons is more electronegative because the nuclear force is greater and/or the atom wants to gain electrons to fill its shell (up and to the right)

Question 17

electron affinity

Answer 17

energy associated with an atom gaining an electron

Question 18

electron affinity trend

Answer 18

more negative electron affinity the higher the attraction is for electrons (kj/mol) trend is up and to the right

Question 19

anion

Answer 19

an ion with a negative charge (gains electrons). larger than a cation

Question 20

cation

Answer 20

an ion with a positive charge (loses electrons). smaller than an anion

Question 21

atomic radius

Answer 21

radius of the atom

Question 22

atomic radius trend

Answer 22

increasing down and to the left of the PT because more shells and EN means the nucleus holds tighter to the electrons and the radius gets smaller

Question 23

ionization energy

Answer 23

the energy required for an element in the gaseous stage to lose an electron

Question 24

Kaddy corner effect

Answer 24

vertical wins over horizontal in periodic trends

Question 25

Ex: which has the most negative electron affinity, C or N? (affinity exceptions)

Answer 25

1) degenerative state? YES 2) do electron configuration (orbital diagram) notice when C and N become aninons (-1 chg) N has 1 pair in its p orbital and 2 unpaired while C has only unpaired electrons i C has a more negative electron affinity since the carbon is entering a more stable state it will give off more energy than nitrogen which is leaving a stable state

Question 26

Degenerate element groups

Answer 26

alkali earth metals (2A), hallogens (7A), 5A

Question 27

Ionic nomenclature

Answer 27

1) the most electropositive element goes 1st 2) most electronegative element goes last and changes suffix (always the nonmetal) 3) # elements in a formula results from balancing the charge

Question 28

Transition metals in ionic molecules

Answer 28

transition metals can have multiple oxidation states (can have different charges)

Question 29

stock system

Answer 29

a roman numeral follows the t metal to show charge

Question 30

latin system

Answer 30

suffix of a t metal changes - ic for larger charge - ous for smaller charge

Question 31

covalent bonding

Answer 31

sharing of electrons (since both elements are non-metals) to reach the noble gas configuration

Question 32

single bond

Answer 32

sharing of 2 electrons between elements

Question 33

double bond

Answer 33

sharing of 4 electrons between elements

Question 34

triple bond

Answer 34

sharing of 6 electrons between elements

Question 35

mono

Answer 35

1

Question 36

di

Answer 36

2

Question 37

tri

Answer 37

3

Question 38

tetra

Answer 38

4

Question 39

penta

Answer 39

5

Question 40

hexa

Answer 40

6

Question 41

hepta

Answer 41

7

Question 42

octa

Answer 42

8

Question 43

nona

Answer 43

9

Question 44

deca

Answer 44

10

Question 45

Molecular Molar Mass

Answer 45

sum of all individual atomic molar masses that make up the molecule

Question 46

Atomic Molar Mass Formula

Answer 46

#atoms of an element x atomic mass

Question 47

% of an element in a molecule formula

Answer 47

(# element)(atomic molar mass)/total molecular molar mass x 100

Question 48

Ex: calculate % N in Fe(NO3)3*5H20)

Answer 48

``` N = 3(14g/mol) = 42g/mol NO3 = 331.8g/mol %N = 42/331.8 x 100 = 12.6% N ```

Question 49

Ex: how many mols hydroxide are there in 10.5 mols of aluminum hydroxide?

Answer 49

hydroxide = OH^-1 chg of Al = +3 --> Al(OH)3 | (10.5 mols Al(OH)3/1)*(3 mols OH/1 mol Al(OH)3) = 31.5 mol OH^-1

Question 50

Ex: how many g of O in 12.5 g of Al(OH)3?

Answer 50

(12.5g/1)*(1 mol Al(OH)3/78.0 g Al(OH)3)*(3 mol O/1 mol Al(OH)3)*(16g O/1 mol O) = 7.69 g O

Question 51

true formula/molecular formula

Answer 51

actual representation of # elements making up a molecule

Question 52

empirical formula

Answer 52

simplest version of the true formula

Question 53

Ex: find the empirical formula for 2.0g copper chloride containing 0.945g Cu and 1.055g Cl

Answer 53

(0.945g Cu/1)*(1 mol Cu/63.5g Cu) = 0.01488 mols Cu (1.055g Cl/1)*(1 mol Cl/35.5g Cl) = 0.0297 mol Cl Cu(0.01488/0.01448)Cl(0.297/0.01448) = CuCl2

Question 54

Ionization energy trend

Answer 54

the amount of energy needed to remove an electron from an atom increases as you go up and to the right on the PT because smaller atoms = higher ionization energy (nucleus has a better hold on electrons)

Question 55

metallic character trend

Answer 55

the ability for an electron to lose an electron (opposite of ionization energy) increases as you go down and to the left on the PT because larger molecules (metals) have less electronegativity (nucleus's hold on the electrons) and want to give their electrons away

Question 56

formal charge

Answer 56

valence electrons - (# lone pairs + 1/2 bonding electrons)

Question 57

Lewis dot structure

Answer 57

an electronic representation of the valence electrons for a given element... electrons are shown as dots and you can have paired or unaired electrons

Question 58

pure covalent bond

Answer 58

same on either side so same EN (= sharing of bonding electrons)

Question 59

bond dipole

Answer 59

unequal sharing of electrons, still shared so still covalent

Question 60

ionic bond

Answer 60

bonding of electrons not being shared because of drastic difference in EN

Question 61

bond lenth

Answer 61

single bonds > double bonds > triple bonds

Question 62

bond strength

Answer 62

single bonds < double bonds < triple bonds

Question 63

radicals

Answer 63

elements that possess 1 unpaired electron

Question 64

incomplete octets

Answer 64

elements that can't reach 8 electrons

Question 65

expansion of octets

Answer 65

elements in the n >/= 3 have at their disposal empty d orbitals to use in bonding... elements possess the ability to share > 8 electrons (so long as n>/= 3)

Question 66

expansion

Answer 66

breaking up lone pairs to increase the # bonds an element can make

Question 67

resonsnace

Answer 67

a delocalization of electrons within a molecule, resulting in more stability for the molecule. drawing a molecule with resonance often deciphers correct structures from the incorrect - a charge (+/-) next to a double bond

Question 68

Valence Shell Pair Repulsion (VSPR)

Answer 68

electron groups (atoms, lone pairs, bonds) naturally repel each other so these electron groups want to be as far away from each other as possible --> 3D geometry