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Chemistry > ⭐️Chemical Bonds > Flashcards

⭐️Chemical Bonds Flashcards

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1
Q

When bonds BREAK

A

Energy absorbed, higher energy state, less stable

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2
Q

What are the 3 types of bonds?

A

Ionic, covalent, metallic

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3
Q

Ionic bond

A

TRANSFER of electrons from balance of 1 atom to balance of another, creating ions

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4
Q

Affinity vs electronegativity

A

Affinity=attraction e have when NOT bonded

Electronegativity= force of attraction and atom has when BONDED

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5
Q

Pauling’s scale of Electronegativity

A

0.0 (no pull, noble gases) to metals, nonmetals and then 4.0 (strongest pull, 7v smallest radius flourine)

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6
Q

If electronegativity diff>1.67?

A

Transfer of e, IONIC

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7
Q

If electronegativity diff

A

Sharing of e, COVALENT

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8
Q

How do you draw Cl when ionically bonded to Na

A

Na+ [Cl]-…an e moved from Na to Cl

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9
Q

Ionic compounds are held together by

A

STRONG electrostatic/electrovalent forces (+) and (-) opposite charges hold metal/nonmetal (usually) together

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10
Q

Ionic compound properties

A 
HIGH MP (strong forces holding +/- together) 
Salts
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11
Q

Bonds

A

Results from the simultaneous attraction of electrons to 2 nuclei

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12
Q

On a periodic table, electronegativity

A

Increases across a row and increases up a column (like affinity/IE)

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13
Q

Ionic Solids

A

Poor conductors, brittle/cleavage, crystalline lattice/NO free moving ions)

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14
Q

Ionic Liquids

A

Good conductors, melted salt (break down crystalline lattice) OR dissolved in solution (aq)…free moving ions

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15
Q

Ionic bonds form when charges are…

A

Opposite and equal (Einstein conservation of energy) to form a shell with the noble gas configuration of the nonmetals period (nonmetals gain)

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16
Q

Empirical formula

A

Simplest whole # ratio by atoms, ionic compounds are only in empirical formulas, (C6H12O6>C1H2O1)

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17
Q

When forming an ionic bond, metals…

A

Lost electrons to non metals

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18
Q

Length of ionic compound

A

Add up 2 radii

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19
Q

Covalent bonds

A

Atoms SHARE a pair/pairs of e… forms MOLECULE

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20
Q

Bond length

A

B/w 2 nuclei, lies on bond axis

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21
Q

Bond axis

A

Connect 2 nuclei

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22
Q

Bond angle

A

Formed by 2 bond lengths

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23
Q

Equal sharing of electrons

A

NON POLAR molecule, symmetrical…diatomic, symmetrical, trigonal planar, tetrahedral

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24
Q

Diatomic molecule

A

NONPOLAR covalent bonds, form NONPOLAR covalent molecules (even dist of e), 2 atoms have same electronegativity/diff=0

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25
Q

Molecular formula vs Lois dot vs vs structural

A

Molecular= N2
Louis dot= Valence dots with circles showing bonds
Structural= Lines showing bonds (#IT NEEDS= #OF LINES) and other electron pairs on opposite ends to show even force/no repel (for non polar)

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26
Q

Symmetrical shape

A

POLAR covalent BONDS but molecule is overall NONPOLAR due to symmetry ex: H-Be-H

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27
Q

When bonds FORM

A

(Potential) Energy released, radius decreases, lower energy state, more stable

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28
Q

Trigonal Planar

A

EXCEPTION TO OCTATE, NONPOLAR symmetry, POLAR no symmetry/double bond on one side, flat, bond angle=120, 0 unshared e-pairs, ex: BH3

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29
Q

Tetrahedral

A

5 atoms 3D, bond angle=109

NONPOLAR symmetrical or POLAR non symmetrical (if 1-3 atoms replaced w another) 0 unshared e-pairs

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30
Q

Methane

A

CH4

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31
Q

Unequal sharing of electrons

A

POLAR molecule, no symmetry, extra e on central atom…linear, bent/v-shape, trigonal pyramid

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32
Q

Bent/v-shape

A

POLAR, bond angle= 104.5, ex: H2O (the large cloud on central O pushes the H’s together…more polar, smaller bond angle) 2 unshared e-pair

33
Q

Trigonal pyramid

A

POLAR, bond angle=107, 4 atoms 3D, ex: NH3, 1 unshared e-pair

34
Q

Trigonal pyramid vs trigonal planar

A

pyramid= unshared pairs of e, always POLAR

Planar=all pairs of e shared, no blob on top, wider bond angle, can be nonpolar

35
Q

Coordinate covalent bonds

A

Central atom shares its UNSHARED PAIR of electrons w H+ (proton tht has no e)….ex: NH4+ (ammonium ion) SEE TABLE E OF POLYATOMIC IONS (NH3+H+>NH4+, H+ needs 2, shares the N’s pair of e)

36
Q

Polar covalent bonds

A

e shared between 2 DIFFERENT atoms

37
Q

Properties of covalent molecules

A

Soft, low mp, poor conductors, generally small (like butter!)

38
Q

Non-polar molecules are only soluble in…

A

Non-polar solvents (benzene, ether) but INSOLUBLE in polar solvents ie H20

39
Q

Network solids/marcromolecules

A

EXCEPTIONS to properties of other covalent molecules, HARD LARGE HIGH MP, but still poor conductors

40
Q

List the 4 network solid exceptions

A

Diamond, graphite, SiC (Silicon Carbide), SiO2 (Silicon dioxide)

41
Q

Hybridization

A

Mix of sublevels to account for # of bonds, ex: C (6, write out e config, 2 unshared pairs (s2p2)>hybridization (electron moves from S to P)>4 unshared pairs (sp3)

42
Q

Linear

A

Bond angle=180, 0 unshared e-pairs, ex: HCl

43
Q

Sigma (o)

A

Single bonds
Lie on bond axis
Strong

44
Q

Pi

A

Made by 2 unhybridized p-orbitals
Lie above/below bond axis/parallel to bond axis
Weaker>easier to break>further from nucleus

45
Q

When there are more bonds…

A

MORE BONDS, MORE ENERGY, CLOSER TOGETHER, HARDER TO BREAK

46
Q

Double bond

A

Pi and sigma (doesn’t matter which is which)

47
Q

Triple bond

A

Pi sandwiching a sigma

48
Q

Polarity

A

Stronger pull on atom w higher en (partial negative charge), protons in nucleus exposed on positive end (partial positive charge), polarity causes molecule-ion attraction CAUSED BY UNEQUAL EN OR UNSHARED PAIRS OF E/UNEQUAL SHARING OF E

49
Q

Molecule-ion attraction

A

Process of how dissolving occurs (ion+polar molecule=dissolve), ex: H2O+NaCl=NaCl (aq)
O end surrounds cation Na+ bc they’re partial neg
H surrounds anion bc they’re partial pos
…Free moving Na+/Cl- ions…GOOD CONDUCTORS

50
Q

Flourine

A

Most electronegative

51
Q

Dipole-dipole forces

A

Intermolecular forces between 2 polar molecules (DOTTED LINE)

52
Q

Intermolecular

A

Between 2 MOLECULES

53
Q

Intramolecular

A

Within the molecule COVALENT BOND

54
Q

Pairs of electrons that bond 2 atoms in a molecule are called

A

Shared pairs (bonding pairs, covalent bonds)

55
Q

Why do electrons in the outer levels of atoms in a molecule spread apart as far as possible?

A

To minimize repulsive forces (e repel each other)

56
Q

How are hybridized orbitals in an atom similar?

A

They are degenerate (have equal energies)

57
Q

How are hybridized orbitals in an atom different?

A

Directions in space (x y z axis)

58
Q

When an sp3 orbital of 1 carbon atom overlaps that of another carbon atom, how many electrons do the two atoms share?

A

2 (1 pair)

59
Q

How many hybrid orbitals can sp3, sp2, and sp have?

A

4, 3, 2 (add)

60
Q

How does the double bond of CH2O (trigonal planar)affect the angle between the 2 single bonds?

A

The angle will be smaller than expected bc the double bond occupies more space then the single bond, pushing them together (

61
Q

A ____ of electrons is formed when an orbital of one atom overlaps and orbital of another atom.

A

Shared pair

62
Q

___ bonds are always formed by sideward or peaked overlap of unhybridized p orbital

A

Pi

63
Q

In single, double, and triple bonds bw 2 carbons, one of the bonds is always a ___ bond

A

Sigma

64
Q

Pi bonds break more easily than sigma bonds bc the electrons forming Pi bonds are (further from/closer to?) the nucleus

A

Further from

65
Q

Single, double, and triple have how many shared pairs of electrons by 2 atoms?

A

Single=1 pair
Double=2 pair
Triple=3 pair

66
Q

Hybridization of orbitals on carbon atom is (H single C triple N 2e)

A

Sp1 (NOT Sp3 bc the pi’s have to be unhybridized p-orbitals)

67
Q

why does water have a bond angle of 104 and not 180?

A

2 unshared pairs of electrons at the oxygen push the hydrogens together, making it polar

68
Q

TEST TIP

A

In NH3, the test might NOT show extra electons on N making it pyramidal so double check

69
Q

EN increases/why…

A

Going right (^ nuclear pull) and doing up (less shielding effect, stronger nuclear pull) F, O, N

70
Q

IMF’s

A

Dipole-dipole and hydrogen bonding, and London dispersion force

71
Q

Hydrogen bonding

A

Dipole-dipole forces between hydrogen of a molecule and highly EN (F, O, N SPECIALLY HIGH EN) of other molecules, HIGHEST IMF, HIGHER MP/BP

72
Q

Dispersion forces

A

Weak forces, magnitude increases with LESS DISTANCE and LAGER MOLECULE SIZE (more forces, more energy to break forces, down column, ^MP, ^SHIELDING EFFECT)

73
Q

Metallic bonds

A

Cations in a sea of mobile electrons, great conductor, high mp, strong, tenacity (malleable/ductile)

74
Q

Van Der Waals radius vs covalent radius

A

Not overlapping (non bonded side) bigger

75
Q

The partially negative side of a polar molecule has a higher…

A

Electronegativity

76
Q

Strongest>weakest bonds/conductivity?

A

1) Metallic (always good conductor)
2) Ionic (strong electrostatic forces, good cond when liquid)
3) Covalent (bad conductors)

77
Q

Exceptions to octate

A

BeH2 (sp, linear, Be has 4 not 8)

BH3/BF3 (sp2, trig planar)

78
Q

When they ask for the hybridization of the orbitals for a molecule with a triple bond…

A

Do NOT include p bonds (Sp3 becomes Sp1)

Chemistry (17 decks)

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