Chemical Bonding Flashcards

1
Q

what is the difference between intra-molecular bonding and inter-molecular bonding?

A

intra-moleculae: the way atoms bond
inter-molecular: the way molecule bonds

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2
Q

what is the octet rule?

A

all atoms, when forming compounds, lose, gain or share electrons- to achieve electron configuration of noble gas.
meaning, to have full valence shell and reach stability.

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3
Q

why boron (B) special?

A

needs only 6 electrons in its valence shell to reach stability.

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4
Q

ionic compounds

A

opposing charged ions are attracted to each other by electrostatic forces.

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5
Q

what is “ionic lattice”?

A

the structure formed in ionic componds.
every negativly charged atom surronded by positive charged atoms, and vice versa.
solid in room temp.

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6
Q

Metallic Bond

A

when 2 or more metal atoms in thier elemental state bonds with each other. they share and lose their valence electrons, those electrons become delocalized.

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7
Q

what are delocalized electrons?

A

Electrons that do not belong or attach to a specific atom, and their location is constantly changing.

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8
Q

what is “metallic lattice”?

A

cations are strongly attracted to the delocalized electrons between them.

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9
Q

what affects the strength of the metallic lattice?

A
  • number of delocalized electrons (the more the merrier)
  • cation charge (more positive, better attraction to the electrons)
    -cation radius (the smaller, the better)
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10
Q

what are the properties of the metallic bond?

A
  • high boiling & melting point
    -conduct electricity & heat
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11
Q

Covalent Bond

A

form between two non-metals
based on sharing electrons from the valence shell.
the electrons that are now shared belong to both atoms (giver & receiver)

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12
Q

How can we know how many electrons are being shared?

A

octet rule- the atoms want to reach stability.

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13
Q

how many electrons can be shared?

A

there are 3 types of bonds:
- single bond (one pair of electrons)
- double bond (2 pairs)
- triple bond (3 pairs)

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14
Q

what is a “lone pair”?

A

electrons in the valence shell, who are coupled with others, and cannot be shared in a covalent bond.

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15
Q

what is the length of a covalent bond?

A

the distance between two bonded nuclei

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16
Q

what is the strength of a covalent bond?

A

the amount of energy required to break the bond

17
Q

what affects the covalent bond length?

A
  • size of atoms
  • bond order (single>double>triple)
  • electronegativity differences between the atoms (polarity).
18
Q

what affects the covalent bond strength?

A
  • bonds of higher order are stronger
19
Q

breaking a double bond vs. single bond

A

breaking a double bond to form a single bond is easier than breaking a single bond.

20
Q

bond polarity

A

electrons that are being shared between atoms with different electronegativity values will be more strongly drawn to the more electronegative atom, which forms unequal distribution of electric charge between the atoms.

21
Q

what is a partial charge?

A

when there is a difference in the electronegativity in a covalent bond, the more electronegativity atom will have constant partial negative charge due to an excess of electrons. the other atom will have constsnt partial positive charge.

22
Q

what is a dipole moment?

A

an electric dipole describes the creation of partial positive and negative charges on opposite atoms of the bond.
-it has a direction represented by an arrow (points to the negataive end of the dipole)

23
Q

what are the types af covalent bond?

A

pure: exect same electronegativity values
non-polar: similar electronegativity values
polar bond: different electronegativity values

24
Q

which type of covalent bond is the strongest?

A

polar bonds

25
Q

what affects the molecule structure?

A
  • amounts of bonds
  • number of lone pairs
26
Q

why carbon oxide is non polar?

A

because of the molecule structure.
the dipole goes to two opposite direction, canceling each other

27
Q

what is a coordinate bond?

A

electron sharing, in which both electron arrives from the same atom (from the lone pair)

28
Q

what is common to both beryllium, aluminium and d block metals?

A

all of them are metals and can form covalent bond.

29
Q

what is the lewis structure?

A

the most common way to draw molecules.
dots= valence electrons
lines= bonds

30
Q

VSEPR theory

A

Valence Shell Electron Pair Repultion
based on the repulsion relations between electrons.

31
Q

what does the VSEPR theory states?

A

stabalized orientation will be that in which thr repultion between electrons is minimized–> the electrons will be located as far as possible from each other.