APCHEM 11th: Ionic and Covalent Bonds

4.0(1)
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/67

flashcard set

Earn XP

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

68 Terms

1
New cards

Levels are …

Sublevels are …

Orbitals are …

Levels are the energy levels/periods/rows, Sublevels are s, p, d, and f, Orbitals are the positions that hold the electrons (# of orbitals half of # of maximum electrons)

2
New cards

Why do ionic bonds tend to have higher melting, boiling points than covalent bonds?

attraction of opposite charge is highly favorable, meaning more energy is needed to break this stability

3
New cards

What is the relationship between an ionic and covalent bond?

Ionic bonds are actually covalent bonds, it's just the electronegativity difference is so much that the electron is transferred completely and not shared

4
New cards

Describe all the covalent bond interactions involving electrons and nucleus

while there's attraction between all electrons and both nuclei, there is also repulsion between nuclei and between electrons, meaning covalent bonds form at the most ideal balance of these forces

5
New cards

What are the x and y axes of the covalent bond graph?

X: internuclear distance in picometers
Y: potential energy (Joules)

6
New cards

Explain the relationship between internuclear distance and potential energy

Up to the ideal/favorable point where the covalent bond fully forms, potential energy decreases due to the increasing nuclei-electron attraction, but afterwards, potential energy increases because the atoms are bonded together yet experience greater repulsion of like charges

7
New cards

How would a Cl-Cl bond compare to an H-H bond on the covalent bond graph?

Cl-Cl will have greater internuclear distance due to more shielding, and the shielding means the valence electrons are farther from both nuclei, so less attraction means greater potential energy

8
New cards

Name different levels of covalent bonds longest to shortest

single-double-triple

9
New cards

Bond energy definition

energy required to separate 1 mole of a certain bond

10
New cards

Lattice energy definition

the energy required to form one mole of a solid ionic compound from its gaseous ions

11
New cards

Coulomb's law

lattice energy = constant * (charge in Coulombs of ion #1)(charge in Coulombs of ion #2) over internuclear distance

12
New cards

Which factor has the bigger effect on lattice energy: internuclear distance or charge?

Charge

13
New cards

Describe the photoelectron spectroscopy graph

the y axis is number of e-, and the x axis is the binding energy that decreases as the electrons move further away from the nucleus

14
New cards

Starting from 1s, describe the gap widths seen on photoelectron spectroscopy graphs

As the energy levels and sublevels increase towards the right, the greatest gaps are between energy levels (EX: 1 to 2) and the smaller gaps are between sublevels (EX: s to p)

15
New cards

What does the Born Haber cycle show?

shows the enthalpy changes that occur in each step of separating/forming an ionic compound

16
New cards

Amount of main, possible steps in the Born Haber cycle and exceptions

5; however, some molecules don't require all steps to occur; EX: In MgS, both atoms are already single as opposed to Na + Cl2

17
New cards

Born Haber cycle step 1; +/- enthalpy change

convert any non-gaseous atoms into gaseous state; endothermic

18
New cards

Born Haber cycle step 2; enthalpy change

separate any diatomic atoms into single atoms; endothermic

19
New cards

Born Haber cycle step 3; enthalpy change

ionization energy is needed to remove the electron(s) from the cation; endothermic

20
New cards

Born Haber cycle step 4; enthalpy change

the anion's electron affinity energy attracts the cation's electron(s); exothermic

21
New cards

Born Haber cycle step 5; enthalpy change

the oppositely-charged gaseous ions now combine to form the final solid compound; exothermic

22
New cards

What do you have to note about electron affinity and ionization energies for atoms that can give away/accept 2 or more electrons?

if atoms give away multiple electrons, those electrons have different ionization energies; so atoms that accept multiple electrons have different electron affinity energies specific to each

23
New cards

If you still have leftover electrons, which atoms should most likely get those extra electrons? (3)

-more electronegative atoms

-atoms that currently have a positive formal charge

-atom that is most furthest down a period starting at period 3

24
New cards

Formal charge equation

of expected valence electrons - actual valence electrons

25
New cards

Polarity definition

the uneven sharing of electrons in molecules due to asymmetrical structure and different electronegativities

26
New cards

Resonance structure definition

structures in which the overall compound charge and position of the atoms stays the same, but the position of some electrons can move around due to not being localized

27
New cards

Hybrid structure 2 aspects

-more stable than the different resonance structures separate

-like a mix of all the resonance structures, so its bond length is between that of single and double bonds

28
New cards

Why can atoms period 3 and beyond expand their octets?

because they have an s, p and d sublevels, not just s and p

29
New cards

Valence Shell Electron Pair Repulsion theory

molecular geometries can be determined thanks to the repulsions between electrons and the greatest minimizations of those repulsions

30
New cards

5 electron domains

linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral

31
New cards

Linear geometry angle measure

180˚

32
New cards

Trigonal planar angle measure

120˚

33
New cards

Tetrahedral angle measure and why?

109.5˚; to minimize repulsions, tetrahedral adopts a multi-plane structure which causes wider angles than what would've been in a planar structure

34
New cards

Trigonal bipyramidal angle measureS

-120˚ between the equatorial

-90˚ between the axial and equatorial

35
New cards

Octahedral angle measure

90˚

36
New cards

What is important to note about lone pairs when figuring out why molecular geometries are the certain shape they are?

lone pairs take up more space and thus have a wider range of repulsion, pushing the other electron pairs closer together

37
New cards

Trigonal planar: 2 molecular geometries and requirements for them

-trigonal planar: all electron pairs are bonded

-bent: 1 nonbonded electron pair

38
New cards

Tetrahedral: 3 molecular geometries and requirements for them

-tetrahedral: all bonded

-trigonal planar: 1 unbonded

-bent: 2 unbonded

39
New cards

If trigonal bipyramidal or octahedral happen to have unbonded electron pairs, where do they go?

the equatorial positions

40
New cards

Trigonal bipyramidal 4 molecular geometries and requirements

-trigonal bipyramidal: all bonded

-seesaw: 1 unbonded

-t-shaped: 2 unbonded

-linear: 3 unbonded

41
New cards

Octahedral: 3 molecular geometries and requirements

-octahedral: all bonded

-square pyramidal: 1 unbonded

-square planar: 2 unbonded

42
New cards

What 6 molecular geometries are symmetrical if all attached atoms are the same in each field?

-linear
-trigonal planar
-square planar
-trigonal bipyramidal
-octahedral
-tetrahedral

43
New cards

Symmetry in regards to trigonal bipyramidal and octahedral structures?

as long as the atoms in the equatorial positions are the same and the atoms in the axial positions are the same, then nonpolar

44
New cards

How to tell if a linear molecular is polar or not?

if atoms on both side of central atom are the same, then nonpolar because of equal dipoles

45
New cards

Polarity arrow trick note #1 for molecule geometries not linear

perform this for every plane of the molecule

46
New cards

Polarity trick #2 for molecular geometries not linear

for each bond, draw the dipole arrow in the appropriate direction

47
New cards

Polarity trick #3 for molecular geometries not linear

assemble the arrows into a cycle; if the cycle can repeat endlessly, it is nonpolar

48
New cards

Hybridization

when an atom is bonding, the s and p orbitals mix together to form hybridized orbitals which correlate with an electron geometry

49
New cards

When does hybridization of an atom not occur?

if atom does not have p orbitals; Ex: H

50
New cards

Along which 3 axes can the 3 p orbitals exist? Their directions?

x and z: horizontal and perpendicular of each other
y: vertical

51
New cards

what is the degrees measure between each of the 3 axes?

90˚

52
New cards

s orbital shape

sphere

53
New cards

p orbital shape

pair of lobes (like an 8)

54
New cards

What are hybrid/degenerate orbitals?

the different variations of the mixing of s and p orbitals (of equal energies) which all merge into one final hybridized structure

55
New cards

sp3 hybridization uses _ out of _ p orbitals and makes _ degenerate orbitals

3; 3; 4

56
New cards

sp3 electron geometry

tetrahedral

57
New cards

How many electrons can each hybridized orbital hold up to?

2

58
New cards

how does sp3 apply to molecules that may have the electron geometry tetrahedral, but molecular geometries of something else?

some hybridized orbitals will not be bonded and will just be holding unbonded electrons

59
New cards

What is joined during sp2 hybridization?

1s + any 2 of the 3 p orbitals (doesn't matter which 2 axes you choose)

60
New cards

sp2 makes _ degenerate orbitals and its electron geometry is

3; trigonal planar

61
New cards

what is a sigma bond?

a type of covalent bond in which the orbitals of different atoms overlap

62
New cards

does the pi bond form between 2 hybridized or non-hybridized p orbitals?

non-hybridized

63
New cards

how do pi bonds form?

pi bonds form perpendicular to sigma bonds and if the non-hybridized p-orbitals are aligned in the same direction

64
New cards

a single bond formed from 2 overlapping hybridized orbitals is a _

sigma bond

65
New cards

generally, a double bond consists of ____

a sigma and pi bond

66
New cards

generally, a triple bonds consists of _

a sigma bond and 2 pi bonds

67
New cards

how many p orbitals does sp hybridization use?

1 out of 3

68
New cards

sp hybridization forms _ degenerate bonds and its electron geometry is

2; linear