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MCAT: General Chemistry > Ch. 3: Bonding and Chemical Interactions > Flashcards

Ch. 3: Bonding and Chemical Interactions Flashcards

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1
Q

What is the octet rule?

A

An atom tends to bond with other atoms so that it has eight electrons in its outermost shell, thereby forming a stable electron configuration similar to the noble gases.

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2
Q

What is a coordinate covalent bond?

A

When the shared electrons between two atoms are contributed by ONLY ONE of the two atoms

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3
Q

Which periodic trend determines whether a covalent bond is polar or nonpolar?

A

Electronegativity

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4
Q

What types of elements form an IONIC bond?

A

Metal and nonmetal

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5
Q

What periodic trend explains the formation of ionic bonds?

A

Electronegativity: ionic bonds form between atoms that have significantly different electronegativities. Example: Sodium and Chlorine

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6
Q

What are characteristic physical properties of ionic bonds?

A

Due to the STRENGTH of the ELECTROSTATIC force between the ionic constituents, ionic compounds have HIGH MP and HIGH BP.

In the aqueous state they are good conductors of electricity. In the solid state they form a cystalline lattice.

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7
Q

What is bond order?

A

The number of electron PAIRS shared between two atoms.

Single bond = bond order of 1
Double bond = bond order of 2
Triple bond = bond order of 3

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8
Q

What is the relationship between bond length and bond energy?

A

Bond length is the distance between two nuclei of atoms in a bond. Bond length DECREASES as the number of shared electron pairs increases.

Bond energy is the energy required to break a bond.

As bond length DECREASES, bond energy INCREASES.

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9
Q

What are the 7 diatomic molecules?

A

N2, O2, F2, Cl2, Br2, I2, and H2

Mnemonic: They form a number 7 on the periodic table (except H2)!

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10
Q

What is the dipole moment equation?

A

p = qd

q is the magnitude of the charge
d is the displacement vector separating the partial charges

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11
Q

What is the name of the reaction that forms coordinate covalent bonds?

A

Lewis Acid-Base reactions

A lewis acid is a compound that will accept a lone pair of electrons. A lewis base is any compound that will donate a pair of electrons to form a covalent bond.

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12
Q

What is the formula for calculating formal charge?

A

formal charge = (normal # e- in valence shell) - (# nonbonding e-) - 1/2(# bonding e-)

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13
Q

What is the difference between sulfate, sulfite, and sulfide?

A

Sulfate: SO4 2-
Sulfite: SO3 2-
Sulfide: S 2-

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14
Q

What is the VSEPR theory?

A

This theory uses Lewis dot structures to predict the molecular geometry of covalently bonded molecules.

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15
Q

What is the ELECTRON pair geometry of a molecule with 2, 3, 4, 5, 6 areas of electron density?

A

2: linear
3: trigonal planar
4: tetrahedral
5: trigonal bipyramidal
6: octahedral

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16
Q

What is the MOLECULAR geometry of a molecule with 3 areas of electron density, one of which is a lone pair?

A

Bent

17
Q

What is the MOLECULAR geometry of a molecule with 4 areas of electron density, one of which is a lone pair?

A

Trigonal pyramidal

18
Q

What is the MOLECULAR geometry of a molecule with 4 areas of electron density, two of which are lone pairs?

A

Bent

19
Q

What is the MOLECULAR geometry of a molecule with 5 areas of electron density, three of which are lone pairs?

A

Bent

20
Q

What is the MOLECULAR geometry of a molecule with 6 areas of electron density, one of which is a lone pair?

A

Square pyramidal

21
Q

What is the MOLECULAR geometry of a molecule with 6 areas of electron density, 4 of which are lone pairs?

A

Bent

22
Q

What are the 3 intermolecular interactions?

A

London Dispersion Forces
Dipole-Dipole
Hydrogen Bonding

23
Q

What is the weakest and strongest intermolecular interaction?

A

Weakest: Lodon Dispersion Forces - van der waals
Strongest: Hydrogen Bonding

24
Q

What are London dispersion forces?

A

Attractive interactions of SHORT LIVED and RAPIDLY shifting dipoles

25
Q

What are dipole-dipole interactions?

A

The positive end of a molecule orients itself with the negative end of different molecule. This arrangement is energetically favorable because of the attractive electrostatic force. This bond is not transient like London dispersion forces.

26
Q

What is a unique physical characteristic of substances with lots of hydrogen bonding?

A

High MP

27
Q

What is considered the hydrogen bond donor vs acceptor?

A

Acceptor: Lone pair of electrons
Donor: Hydrogen atom

MCAT: General Chemistry (11 decks)

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