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Chemistry R120 > Chapter 8: Basic Concepts of Chemical Bonding > Flashcards

Chapter 8: Basic Concepts of Chemical Bonding Flashcards

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1
Q

What are the 3 types of chemical bonds?

A

ionic | covalent | metallic

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2
Q

What are ionic bonds?

A

electrostatic attractions between oppositely charged ions

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3
Q

What are covalent bonds?

A

atoms sharing electrons

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4
Q

What are metallic bonds?

A

electrons are free to move from one atom to another

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5
Q

What is the octet rule?

A

atoms tend to gain/lose/share electrons until they are surrounded by 8 electrons (want to be like noble gas)

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6
Q

What does the electron configuration of a noble gas consist of?

A

FULL s and p orbitals

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7
Q

What is the usual pairing of an ionic bond?

A

a metal from 1A/2A and a nonmetal

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8
Q

What does an atom’s ionization energy indicate/affect electron transfer?

A

indicates how easily an atom can give up an electron

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9
Q

What does an atom’s electron affinity effect electron transfer?

A

measures how much an atom wants to gain an electron

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10
Q

What is electron transfer?

A

when one atom readily gives up an electron (low IE) and the other electron readily accepts an electron (high EA)

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11
Q

What are the 3 characteristics of ionic substances?

A

brittle | high melting point | crystalline

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12
Q

What type of process (endothermic or exothermic) is loss of electrons from an atom?

A

endothermic

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13
Q

What type of process (endothermic or exothermic) is gaining of electrons of an atom?

A

exothermic

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14
Q

Why are ionic compounds stable?

A

attraction between oppositely charged ions draws them closer together = releasing energy (exothermic) = forms a lattice

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15
Q

What is lattice energy?

A

energy needed to completely separate 1mol of a solid ionic compaound into its gaseous ions

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16
Q

What describes the stability of a lattice structure?

A

lattice energy

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17
Q

What type of process (endo/exo) is forming ionic compounds?

A

exothermic

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18
Q

What are the 3 things that the lattice energy magnitude of a solid depend on?

A

charges of the ions (mainly) | ionic size and their arrangement in the solid

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19
Q

What is the relationship between lattice energy and the size and radii of the ions?

A

lattice energy increases as ionic size increases and ionic radii Decreases and distance between ions increase

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20
Q

What is the limitation/restriction to adding/removing electrons from s and p elements

A

s-block: can only remove e- from valence shell | p-block: can only add e- to valence shell = otherwise its energetically unfavorable

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21
Q

How are electrons added or removed to/from transition metals?

A

e- from valence shell are lost first | subsequent removal comes from d-orbital electrons

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22
Q

How could atoms have noble-gas electron configurations?

A

by sharing “borrowing” electrons

23
Q

What is a covalent bond?

A

chemical bond formed by sharing a pair of electrons

24
Q

How do covalent bonds stick if it is the sharing of electrons?

A

the shared electrons (any 2 electrons) are in between the atoms’ nuclei, the attractive forces between electron-nucleus “hold” the bond together

25
Q

What are non-bonding pairs in the Lewis Dot Structure?

A

lone pairs

26
Q

What is bond polarity?

A

measure of how equally/unequally the electrons in any covalent bond are shared

27
Q

What is a non-polar covalent bond?

A

electrons are shared equally

28
Q

What is a polar covalent bond?

A

one of the atoms exerts a greater attraction for the bonding-electrons than the other atom

29
Q

What separates a polar covalent bond from an ionic bond?

A

difference in magnitude of attraction between an atom for the bonding electrons compared to another atom

30
Q

What is electronegativity?

A

ability of an atom in a molecule to attract electrons to itself

31
Q

What determines the type of chemical bond in a molecule?

A

the electronegativity of an atom

32
Q

What 2 things affect an atom’s electronegativity?

A

ionization energy and electron affinity

33
Q

What must the EA and IE of an atom be in order to have an increase in electronegativity?

A

EA must be (-) and IE increases = resists having its e- taken away

34
Q

Who is Linus Pauling?

A

developed the first and most widely used electronegativity scale based on thermochemical data

35
Q

What is the periodic TREND for electronegativity?

A

increases left –> right | increase UPward a group

36
Q

What is the electronegativity in atoms with a non-polar bond?

A

similar electronegativities

37
Q

What is the electronegativity in atoms with a polar-bond?

A

one of the atoms is MORE electronegative than the other and the electron density cloud shifts more toward the more electronegative atom

38
Q

What is the electronegativity in atoms with a ionic bond?

A

difference in electronegativity MUST BE > 2

39
Q

What are polar molecules attracted to and why?

A

ions, due to their partial charges

40
Q

What is a dipole?

A

whenever 2 opposite electrical charges are separated by a distance

41
Q

What is a dipole moment (µ)?

A

quantitative measure of the magnitude of a dipole

42
Q

What are the 3 characteristics of molecular compounds?

A

low melting point | low boiling point | non-electrolyte behavior in water

43
Q

What is expected when covalent bonding is dominant?

A

compounds exists as molecules

44
Q

How can we distinguish between an ionic and covalent bond?

A

use the differences in electronegativity

45
Q

What is a formal charge?

A

potential charge the atom would have if each bonding e- pain in the molecule were shared equally between 2 atoms

46
Q

What are the 2 ways to identify the dominant Lewis structure?

A

formal charges are closest to 0 | (-) charges reside on the most electronegative atoms

47
Q

What are resonance structures?

A

placement of atoms are the same but vary in placement of electrons

48
Q

What bonds do resonance structures only occur with?

A

double bonds

49
Q

What are the 3 exceptions to the octet rule with molecules and polyatomic ions?

A

odd # electrons | atom has fewer than 8 valence e- | atom is hypervalent

50
Q

What is hypervalent?

A

atom has more than 8 valence electrons

51
Q

What are hypervalent molecules formed only for?

A

central atoms on Period 3 and below due to their large size

52
Q

What is the stability of a molecule related to?

A

the strength of its covalent bond

53
Q

What happens as the number of bonds between 2 atoms increase to the bond distance, bond enthalpy and bond strength?

A

shorter distance = atoms closer together = increase in bond enthalpy = increase bond strength

Chemistry R120 (18 decks)

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