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Chemistry > Chapter 11&12 bonding (6.2 APC) > Flashcards

Chapter 11&12 bonding (6.2 APC) Flashcards

0
Q

What kind of electrons are involved with chemical bonding?

A

Valence electrons

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1
Q

What is a chemical bond?

A

The force of attraction that hold atoms or ions together in a chemical substance.

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2
Q

Types of bonds

A
  • ionic
  • compound
  • covalent
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3
Q

Ionic bond

A

Metal + non-metal
Electrons are transferred
1.7 EN

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4
Q

Covalent Bond

A

Non-metal + non-metal
Electrons are shared equally and non equally
0-0.4 0.4-1.7 EN

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5
Q

Metallic Bond

A

Metal + metal
Sea of electrons
1.7< EN

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6
Q

When electrons are shared equally

A

Polar

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7
Q

Non polar

A

When electrons are shared equally

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8
Q

Ionic bonds are commonly called

A

Salts

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9
Q

Ionic bonds form when…

A

Electrons transfer from one atom to another due to large differences in electromagnitivity and ionization energy

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10
Q

Ionic bonds are isoelectric with noble gases..

A

When atoms gain or lose electrons to have the same amount as the nearest noble gas.

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11
Q

Most stable valence of electrons is…

A

An octet (8)

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12
Q

Which element is the exception of not having an octet?

A

He, 2 valence electrons

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13
Q

In ionic bonds, metals..

A

Lose electrons to be like the closest noble gas (isoelectric)

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14
Q

In ionic bonds, nonmetals…

A

Gain electrons to become like the closest noble gas (isoelectric)

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15
Q

If the EN is greater than 1.7, then…

A

Atoms have been transferred

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16
Q

EN is how well an atom ______ _______

A

Attracts electrons

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17
Q

When a metal loses one or more electrons, it become a…

A

Positively charged ion (Cation)

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18
Q

When a nonmetal gains one or more electrons, it becomes a…

A

Negatively charged ion (anion)

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19
Q

Cation

A

Positively charged ion

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20
Q

Anion

A

Negatively charged ion

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21
Q

Electrostatic attraction

A

The attraction between oppositely charged ions.

22
Q

Electrostatic attraction makes….

A

Atoms stick together in an ionic bond.

23
Q

Polyatomic ions

A

Groups of atoms(molecules) that have an overall charge and act like a single ion

24
Properties of ionic compounds:
- form crystals (lattices) - very brittle - extremely high melting points - soluble in water and conduct electricity
25
Lattice energy
A measure of his energy is released when the bonds form
26
Covenant bonds are commonly called....
Molecules
27
Covenant bond formation: covalent bonds involve...
The sharing of electrons between two nonmetals
28
Electrons are always shared __ _____
In pairs
29
If EN is less than 0.4, then...
Electrons are shared with each other equally (no polar covenant bond)
30
If the EN is more than 0.4 (but less than 1.7, because that is an ionic bond), one atom is pulling the electrons closer to itself, so....
One atom will become partially negative and another positive creating electrons to be shared unequally (polar)
31
Electron density
Atoms with the biggest electronegativity (negative)
32
Lewis structure, remember:
- Hydrogen only needs 2 electrons - boron only needs 6 electrons - carbon always goes I'm the middle - hydrogen always goes on the outside - the element with the lease electromagnitivity (furthest from fluorine) goes in the middle
33
Atomic radius
As we move down a group the sizes of atoms increase As we move across a period the sizes decrease Smallest (helium) Largest (cesium)
34
Ionization energy (IE)
The minimum energy required to remove an electron from a gaseous atom or ion ~ tells how strongly an atom holds onto its outermost electrons
35
Low IE
More likely to lose electrons and form cations during chemical changes
36
High IE
Atom gains electrons and form anions or no ions at all
37
Lowest IE energy is associated with
Larger atoms (lower left corner of periodic table)
38
The highest IE correspond with
The smaller atoms (upper right)
39
The greater number of protons present on an ion, the ______
Stronger the attractive force on the electron cloud (the smaller the atom)
40
Electronegativity
The relative ability of a bonded atom to attract shared electrons to itself
41
Atoms with high EN tend to
Pull bonded electrons closer to their nuclei Pulled further away for lower EN values
42
Atoms and EN
Smaller atoms have higher EN | larger atoms have lower EN
43
Shielding effect
The reduction in the nuclear charge felt by a valance electron
44
Photoionization
When a valance electron is completely removed resulting in a creation of an ion
45
Involves the use of a device that focuses a monochromatic beam of X-rays at a solid sample
Photoelectron Spectroscopy
46
PES spectrum peaks
``` S = 2 P = 6 D = 10 ```
47
Ionic (ap def)
Electrostatic attraction force between oppositely charged ions produced when a metal armor transfers one or more electrons to a non-metal atom
48
Lewis structures (electron dot diagrams) how to
1. Find total number of valence electrons 2. Put least EN atom in the center 3. Put two electrons between atoms to form a chemical bond, fluorine and oxygen most = EN (hydrogen always outside) 4. Complete octets on the outside atoms (hydrogen only needs 2) 5. If central atom doesn't have an octet, move some from the outer atoms to form double or triple bonds
49
Lewis structure important points
1. As each element in a family has the same number of valence electrons, the Lewis structure for those elements has the same number of dots 2. For metals, the total number of dots represents the number of electrons that each atom loses when forming a cation 3. For a nonmetal, the number of unpaired dots represents either the number if electrons that arid must gain when forming an anion, or the number of the electrons the atoms must share to complete its octet when forming covalent bonds
50
When drawing lewis structures for monatomic metals in groups 1, 2, and 13...
Do not include any dots The element symbol is usually enclosed in square brackets with the cations charge written outside the brackets on the top right
51
When drawing lewis structures for monatomic nonmetals in groups 15, 16, and 17...
Lewis structures for their anions all include four pairs of dots surrounding the element symbol enclosed in square brackets with the appropriate negative charge written outside the brackets
52
Lone-pair electrons
Non-bonding electrons

Chemistry (7 decks)

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