Atoms, Elements and Compounds

Negative

Neutral

Positive

Variable depending on the electrons

It is a highly reactive metal

It is a colorless, odorless gas

It forms diatomic molecules like $\text{Cl}_2$

It is a liquid at room temperature

Sulfur

Silicon

Iron

Argon

Only protons

Only neutrons

Protons and neutrons

Protons and electrons

Group III, Period 2

Group III, Period 3

Group I, Period 3

Group III, Period 4

24

20

44

64

2+

6+

2-

6-

$Mn^{2+}$

$Fe^{3+}$

$Cr^{2+}$

$Co^{2+}$

$4s < 3d < 4p < 5s < 4d$

$3d < 4s < 4p < 4d < 5s$

$4s < 4p < 3d < 4d < 5s$

$4s < 3d < 4p < 4d < 5s$

The number and arrangement of valence electrons.

The number of neutrons in the nucleus.

The relative atomic mass of the element.

The ratio of protons to neutrons.

$^{39}_{20}Ca$

$^{39}_{19}K$

$^{20}_{19}K$

$^{19}_{39}Y$

The number of neutrons in the nucleus

The total number of protons and neutrons

The number of protons in the nucleus

The total number of particles in the atom

3

4

7

10

Only protons

Only neutrons

Both protons and neutrons

Both protons and electrons

Atomic number; Mass number

Mass number; Atomic number

Neutron number; Proton number

Electron number; Proton number

Hydrogen-1

Oxygen-16

Carbon-12

Helium-4

The number of nucleons

The number of protons

The number of neutrons

The mass of the atom in grams

12 g

13 g

13.003 g

12.011 g

They have the same number of valence electrons

$^{81}Br$ has a higher boiling point than $^{79}Br$ in elemental form

They occupy the same position in the Periodic Table

$^{81}Br$ has a larger atomic volume than $^{79}Br$

94

96

98

100

$N^-$

$N^{2-}$

$N^{3-}$

$N^{3+}$

$PbNO_3$

$Pb(NO_3)_2$

$Pb_2NO_3$

$Pb_2(NO_3)_2$

$2+$

$6+$

$2-$

$6-$

1

2

2, 1

2, 8

$KS$

$KS_{2}$

$K_{2}S$

$K_{2}S_{3}$

1

2

3

4

$CuO$

$Cu_{2}O$

$CuO_{2}$

$Cu_{2}O_{2}$

Very soluble in water.

Insoluble in water.

A liquid at room temperature.

A good conductor of electricity in the solid state.

High melting and boiling points.

The existence of a regular crystal shape.

Electron density maps obtained from X-ray diffraction showing discrete regions of electron density.

The fact that the substance is brittle.

It becomes more exothermic from $F^{-}$ to $I^{-}$ as the ions get larger.

It becomes less exothermic from $F^{-}$ to $I^{-}$ as the charge density decreases.

It remains constant because they all have a charge of $-1$.

It is zero for all halide ions as they do not react with water.

Conductivity in molten state

Very high melting points

Weak forces between molecules

Hard and brittle

Ionic

Metallic

Single covalent

Double covalent

$NaCl$

$H_2O$

$O_2$

$C$ (diamond)

The total number of protons

The number of electrons needed to fill the outer shell

The atomic mass

The number of neutrons

End-to-end overlap of $s$ orbitals

End-to-end overlap of $p$ orbitals

Side-to-side overlap of $p$ orbitals

Overlap of an $s$ and a $p$ orbital

2

4

6

8

Iodine

Silicon

Dry ice ($CO_2$)

Sulfur

1

2

2.5

3

$CO_3^{2-}$

$NO_3^-$

$SO_3^{2-}$

$BF_3$

All covalent compounds are insoluble in water.

Polar covalent compounds are generally soluble in non-polar solvents.

Non-polar covalent compounds are generally soluble in non-polar solvents due to induced dipole-induced dipole interactions.

Giant covalent structures like diamond are soluble in organic solvents.

Valence electron

Proton

Conduction electron

Free electron

Magnetic attraction

Electrostatic attraction

Gravitational attraction

Nuclear attraction

It conducts electricity when molten

It is a liquid at room temperature

It has a high melting point

It is composed of $SiO_2$ molecules

Ionic bonds between copper and zinc

Covalent bonds between copper and zinc

Metallic bonds in a mixture of copper and zinc

Weak forces between copper and zinc molecules

$SiO_2$ contains stronger covalent bonds than $CO_2$.

$SiO_2$ is a giant macromolecule, while $CO_2$ is a simple molecule.

Silicon is a metal and carbon is a non-metal.

$SiO_2$ has ionic character while $CO_2$ is purely covalent.

Brass

Diamond

Ice

Solid Carbon Dioxide

Low melting point

High solubility in non-polar solvents

High melting point due to many strong covalent bonds

High electrical conductivity in the solid state (for all examples)

They are approximately the same because both centers are $sp^3$ hybridized.

Diamond's angle is $120^\circ$ while $SiO_2$ is $109.5^\circ$.

Diamond's angle is $109.5^\circ$ while $SiO_2$ is $180^\circ$ because it is linear.

Diamond's angle is smaller because carbon is a smaller atom.

A single layer of carbon atoms arranged in a hexagonal lattice.

A series of stacked layers of carbon atoms with no bonding between them.

A cage-like molecule containing 60 carbon atoms.

A 3D network of carbon atoms where each atom is bonded to three others.

The $K^+$ ion is larger than the $Na^+$ ion, so the attraction to the delocalized electrons is weaker.

Sodium has more delocalized electrons per atom than Potassium.

Potassium is more reactive than Sodium, making its bonds less stable.

Sodium has a higher atomic mass, requiring more energy to melt.