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Chemistry 11 > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is the name of this VSEPR Shape?

A

Bent 90-109 degrees

2 electron pairs

2 lone pairs

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2
Q

What is the name of this VSEPR Shape?

A

Bent 90-109 degrees

2 electron pairs

1 lone pair

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3
Q

___ is the smallest particle of an ellement that retains all the chemical properties of that element.

A

Atom

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4
Q

A ______ is any electrically neutral group of atoms that is held together tightly enough to be considered a single particle.

A

molecule

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5
Q

a metal reacts with a non-metal, electrons are transferred from metal to non-metal

A

Ionic Bond

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6
Q

When this happens the atoms of the non-metal become negatively charged ions, while atoms of the metal become positively charged ions.

A

Ionic Bonding

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7
Q

When an atom has the same elctron arrangement as another atom, the two atroms are referred to as ______.

A

Isoelectronic

ex. Na+ is isoelectronic with Ne

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8
Q

What is this VSEPR Shape?

A

Linear 180 degrees

2 electron pairs

0 lone pairs

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9
Q

____ the attraction between the atoms in a molecule.

A

Chemical Bonds

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10
Q

Chemical bond can form when….

A

electrons are simultaneously attracted to each others nuclei. Only valence electrons are involved in bonding.

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11
Q

____ are more stable than the isolated atoms from which they are formed

A

molecule

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12
Q

stability of an atom with 8 valence electrons

A

Stable Octet

**All noble gases except He, have a stable octet and so are very stable and relatively inert with respect to bonding with each other/ with other elements.

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13
Q

when electrons are shared between two atoms

A

Covalent bond

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14
Q

What is this VSEPR Shape?

A

Octahedral 90 degrees

6 electron pairs

0 lone pairs

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15
Q

resembles the electron dot diagram, except that single lines are used to represent each shared pair of electrons and dots are used to represent electrons not involved in bonding.

A

Lewis Dot Diagram

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16
Q

A ________results when electrons are not shared equally.

A

Polar Covalent Bonding

ex. HCl

sharing is not equal, Cl atom has a stronger attraction for the shared pair of electrons that does the H atom. This makes the Cl atom slightly NEGATIVE and the H atom slightly POSTIVE

17
Q

δ what is this used to represent?

A

That one atom has a slight positive/ negative charge only used for polar covalent bonding

18
Q

A ______ is formed when two pairs of electrons are shared between two atoms

A

Double Covalent Bond

19
Q

Formed when three pairs of electrons are shared between two atoms

A

Triple Covalent Bonding

20
Q

A bond in which both electrons of the sthared pair come from only one of the bonded atoms

A

Coordinate Covalent Bond

21
Q

What is this VSEPR Shape?

A

Tetrahedral 109.5 degrees

4 electron pairs

0 lone pairs

22
Q

What is this VSEPR Shape?

A

Trigonal Bipyramidal 90 degrees

120 degrees

180 degrees

4 electron pairs

0 lone pairs

23
Q

What is this VSEPR Shape?

A

Trigonal Planar

120 degrees

3 electron pairs

0 lone pairs

24
Q

A ____ is simply an extreme case of polar covalent bonding

A

Ionic

25
Q

A quantitative measure of an atom’s electron attracting ability

A

Electronegativity

26
Q

The ____ the electronegativity value, the ____ the attraction of electrons

A

higher, greater

lower, less

27
Q

Core Atom Exceptions to Octet Rule

A
  1. Be
  2. B
  3. S
  4. P
  5. Sn
28
Q

What is the ΔEneg for Pure Covalent Bonds?

A

ΔEneg= <0.5

NO EXCEPTIONS

29
Q

If Carbon has a electronegativity of 2.55 and Chlorine of 3.16 which one would be slightly more negative

A

Chlorine

*PLACE A for each atom δ- for each atom!!

30
Q

for a molecule to be polar…

A
  1. molecule must contain at least 1 polar bond
  2. molecule must be assymetrical

In the picture this molecule contains at least one polar bond and it is assymetrical (because one side is negative and the other positive)

****BOTH CONDITIONS MUST BE MET FOR IT TO BE POLAR***

31
Q

Can a pure covalent bond be polar?

A

No because neither atom can be slightly positive/negative and therefore it does not even satisfy the first requirement to have a polar bond.

32
Q

Do you draw a VSEPR diagram for ionic bonds?

A

No, this is because ionic bonds are attracted to each other because of attraction of opposites and does not have a specific shape in which they form. They are flat.

Chemistry 11 (3 decks)

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