Chemistry: Atomic Structure, Bonding, and Periodicity

4

2, 2

2, 8

1, 3

The shell furthest from the nucleus

The shell closest to the nucleus

The middle shell

All shells fill at the same time

17

35

18

52

Mass number

Number of neutrons

Atomic number

Number of shells

8

16

0

24

2, 8, 4

2, 4, 8

4, 8, 2

14

Proton

Neutron

Electron

Nucleus

15

18

21

13

$Mg^{2+}$

$K^{+}$

$Na^{+}$

$Al^{3+}$

Calcium

Argon

Potassium

Titanium

S

So

Sd

Na

High melting points

Formed between metals and non-metals

Usually poor conductors of electricity

Exist only as solids

Valence electrons

Protons

Electron shells

Neutrons

-1

0

+1

+11

Result A

Result B

Result C

Result D

$+1$

$-1$

$0$

$+2$

$He$

$Ne$

$N_2$

$CO_2$

They increase because the atoms get heavier.

They decrease because the metallic bond gets weaker as the ions get larger.

They stay the same because they all have one valence electron.

They increase because the number of delocalized electrons increases.

The number of neutrons in the atoms.

The degree of overlap between atomic orbitals and the distance between nuclei.

The total mass of the molecule.

The color of the substance.

Linear

Square Planar

Tetrahedral

Pyramidal

Number of protons

Number of electron shells

Number of valence electrons

Atomic mass

Oxygen

Nitrogen

Carbon

Sodium

Highly reactive

Very unreactive

Liquid at room temperature

Good conductor of heat

Clouds

Waves

Shells

Paths

$A_{2}B$

$AB$

$AB_{2}$

$A_{3}B$

Process 1: Ionic; Process 2: Metallic

Process 1: Covalent; Process 2: Ionic

Process 1: Metallic; Process 2: Covalent

Process 1: Ionic; Process 2: Covalent

The presence of different-sized atoms in Model B disrupts the regular layers, making it harder for them to slide over each other.

The atoms in Model B are held together by strong covalent bonds rather than metallic bonds.

The different-sized atoms in Model B have a higher number of protons, creating a stronger magnetic pull between layers.

The alloy atoms in Model B are spaced further apart, which allows the material to absorb more force without bending.

Metallic bonding with delocalized electrons.

Ionic bonding between carbon ions.

Giant covalent lattice where each carbon is bonded to four others.

Simple molecular structure held by weak Van der Waals forces.

1

2

3

4

$Cl^{-}$

$Li^{+}$

$Al^{3+}$

$K^{+}$

They all conduct electricity

They are all allotropes of carbon

They all have high melting points

They are all slippery

1:1

1:2

2:1

4:1

2

4

6

8

Graphite

Wax

Plastic

Ice

Silicon is a metal, so its oxide ($SiO_2$) has a much higher melting point than the non-metal oxide ($CO_2$).

Carbon dioxide consists of molecules held together by strong ionic bonds, while silicon dioxide is held by covalent bonds.

Silicon dioxide is a giant covalent structure that requires significant energy to break its strong bonds, whereas carbon dioxide consists of small molecules held by weak forces.

Silicon dioxide molecules are much larger and heavier than carbon dioxide molecules, which prevents them from melting easily.

They are all made of carbon.

They consist of billions of atoms bonded in a continuous network.

They are all slippery and soft.

They all contain delocalized electrons.

1

2

3

4

The delocalized electrons between the layers absorb all the thermal energy, causing only the vertical gaps to expand.

The distance between layers is so large that any increase in kinetic energy causes the atoms to vibrate only in a vertical direction.

The strong covalent bonds within the layers resist the movement of atoms, whereas the weak forces between the layers allow them to move further apart as temperature increases.

The hexagonal rings within the layers are rigid and cannot expand, forcing all thermal expansion to occur between the layers.

The bonds in graphite layers are shorter because they have partial double-bond character.

The bonds in diamond are shorter because it is a harder material.

They are the same length because they are both carbon-carbon bonds.

The bonds between the layers of graphite are the shortest.

Because the number of atoms in one crystal is essentially infinite on an atomic scale.

Because the atoms themselves are much larger than other atoms.

Because they only form very large visible crystals.

Because they have very high atomic masses.