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Chemistry > Bonds & Details > Flashcards

Bonds & Details Flashcards

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0
Q

Covalent bond

When the electrons are not shared equally, it is called?

A

Electrons shared between 2 atoms

The bond is considered polar

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1
Q

Ionic bond?

Why does the bond stay together?

A

Electrons are taken and given away, resulting in charged particles.
Bond stays together due to electrical attraction

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2
Q

Covalent bonds result in what shapes?

Ionic bonds?

A

Covalent- VSEPR shapes

Ionic- crystals

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3
Q

Are acids an ionic or covalent bond?

What does the hydrogen act like?

A

Ionic

Like a cation

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4
Q

Cation vs anion

A

Cation- the positively charged ion

Anion- the negatively charged ion

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5
Q

What do covalent bonds form, while ionic bonds do not?

A

Molecules

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6
Q

Valence electron

A

An electron in the outermost energy level of an atom that can participate in bonding

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7
Q

Unshared pair (lone pair)

A

A nonbonding pair of electrons in the valence shell of an atom.

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8
Q

Single bond

A

A bond in which two atoms share one pair of electrons

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9
Q

Triple bond

A

Covalent bond in which 2 atoms share 3 pairs of electrons

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10
Q

Double bond

A

Covalent bond in which 2 atoms share 2 pairs of electrons

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11
Q

Resonance structure

A

Possible Lewis structure of a molecule for which more than one Lewis structure an be written

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12
Q

Lewis structure

A

A structure in which atomic symbols represent nuclei and inner-shell electrons and in which dots are used to represent valence electrons

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13
Q

What does VSEPR theory predict?

A

The 3-D formation of a molecule, shape of the molecule

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14
Q

The shape of molecules that contain only 2 atoms is

A

linear

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15
Q

Why is there not resonance structures of CO despite its triple bond?

A

There is no other way of making a different structure

16
Q

Electronegativity

A

Tendency of an atom in a molecule to attract shared electrons to itself

How good an atom is at attracting electrons to its nucleus

17
Q

Is “polar ionic” possible? Why or why not

A

No, Because in order to be polar, the en has to be less than 2 and greater than .5. If a bond is ionic, it will have an electronegativity greater than 2 meaning that it will never be polar.

18
Q

When should you use electronegativity to calculate whether or not a bond is polar?

A

When it is a covalent bond

19
Q

What does VSEPR stand for?

A

valence shell electron pair repulsion

20
Q

Why are nonpolar covalent bonds not common?

A

Because one atom usually attracts electrons more strongly than the other

21
Q

Nonpolar covalent bond

A

Attraction between two atoms in which bonding electrons are shared equally between the atoms

22
Q

Polar covalent bond

A

Attraction between two atoms in which bonding electrons are localized on the more electronegative atom

23
Q

Where on the periodic table is electronegativity the highest?

A

Upper right hand side

24
Q

Where on the periodic table is electronegativity the lowest?

A

Bottom left hand side

25
Q

Dipole molecule

A

One that has a partial positive charge at one end and a partial negative charge at the opposite end

26
Q

In general, if the difference in electronegativity between 2 atoms is between 0 & .4 the bond formed is…

A

Non polar covalent

27
Q

If the difference in electronegativity between 2 atoms is between .4 and 2 the bond formed is…

A

Polar covalent

28
Q

If the electronegativity difference between 2 atoms is greater than 2 the bond formed is…

A

Ionic

29
Q

If one atom has more electronegativity, then it is partially ____

A

Negative

30
Q

The positive atoms shown in dipole moment arrows go where?

A

Towards the partially negative atom because it has more electronegativity

31
Q

What is meant by unequal sharing of electrons in a polar bond?

A

More electronegative atoms pull on shared electrons more than the other atom so the charge is not evenly distributed -> opposite sides -> opposite charges

32
Q

If their are lone pairs on the center element of the covalent bond, is it a polar or nonpolar molecule?

A

Polar

33
Q

No lone pairs. Polar or nonpolar molecule?

A

Nonpolar

34
Q

If dipole moments cancel out, is the molecule polar or nonpolar?

A

Nonpolar

35
Q

If the dipole moments don’t cancel & there are lone pairs, the molecule is…

A

Polar

36
Q

Right on the periodic table, what happens?

A

Nucleus gets bigger so it’s easier to steal electrons (more en)

37
Q

Down on the periodic table, what happens?

A

Further away from the nucleus, more energy levels (less en)

38
Q

Molecules have a certain ____ based on how the electrons repel each other

A

Shape

Chemistry (16 decks)

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