Unit 2: Ions, Ionic and Molecular Compounds, and Changes of State

Physical and Chemical Changes, Ions, and Compounds

Introduction

This unit covers the fundamental concepts of ions, ionic and molecular compounds, and changes of state. Understanding these topics is essential for grasping the basics of General, Organic, and Biological (GOB) Chemistry.

Chemistry and Valence Electrons

Structure of the Atom

• Atoms consist of a nucleus (containing protons and neutrons) surrounded by electrons.

• Protons (p+): Positively charged particles in the nucleus.

• Neutrons (n0): Neutral particles in the nucleus.

• Electrons (e-): Negatively charged particles in orbitals around the nucleus.

The arrangement of electrons, especially the valence electrons (those in the outermost shell), determines the chemical properties of an element.

Valence Electrons and Energy Levels

• Valence electrons have the highest energy and are farthest from the nucleus.

• The number of valence electrons is crucial for chemical reactivity and bonding.

• Elements in the same group (vertical column) of the periodic table have the same number of valence electrons.

Electron Dot Symbols (Lewis Symbols)

• Valence electrons can be represented using Lewis dot symbols.

• Each dot represents a valence electron placed around the element symbol.

• Example: For carbon (C), which has 4 valence electrons: C with four dots around it.

Ions and Ionic Charges

Formation of Ions

• Cations: Positively charged ions formed when atoms lose electrons (usually metals).

• Anions: Negatively charged ions formed when atoms gain electrons (usually nonmetals).

• The charge of an ion is shown as a superscript after the element symbol (e.g., Na+, Cl-).

Predicting Ionic Charges

• Group 1A metals: +1 charge

• Group 2A metals: +2 charge

• Group 7A nonmetals: -1 charge

• Group 6A nonmetals: -2 charge

• The charge can often be predicted from the group number.

Octet Rule

• Atoms tend to gain, lose, or share electrons to achieve a full set of eight valence electrons (an octet), similar to the noble gases.

• Helium is stable with two valence electrons (a duet).

Ion Symbols and Names

• For cations, the ion symbol and Lewis dot symbol are the same (e.g., Na+).

• For anions, the symbol shows the element and the number of gained electrons (e.g., Cl-).

• Cation names are the same as the element (e.g., magnesium ion).

• Anion names are formed by taking the root of the element and adding -ide (e.g., chloride ion).

Table: Common Ions and Their Charges

Element	Symbol	Charge
Sodium	Na+	+1
Magnesium	Mg2+	+2
Chlorine	Cl-	-1
Oxygen	O2-	-2

Ionic Compounds

Properties of Ionic Compounds

• Composed of cations and anions held together by electrostatic forces (ionic bonds).

• Have high melting points and are usually solid at room temperature.

• Are electrically neutral overall (total positive charge equals total negative charge).

Writing Ionic Formulas

• The formula shows the simplest ratio of ions that results in a neutral compound.

• Subscripts indicate the number of each ion in the compound.

• Example: Magnesium chloride is MgCl2 because two Cl- ions are needed to balance one Mg2+ ion.

Table: Subscripts in Formulas

Compound	Cation	Anion	Formula
Magnesium chloride	Mg2+	Cl-	MgCl2
Calcium oxide	Ca2+	O2-	CaO
Aluminum oxide	Al3+	O2-	Al2O3

Naming Ionic Compounds

• Name the cation first, then the anion.

• For metals with variable charges (transition metals), use Roman numerals to indicate the charge (e.g., FeCl2 is iron(II) chloride).

• Monatomic anions are named with the root of the element plus -ide (e.g., oxide, sulfide).

Changes of State and Temperature Scales

States of Matter

• Solids: Definite shape and volume; particles are closely packed and vibrate in place.

• Liquids: Definite volume but no definite shape; particles are close but can move past each other.

• Gases: No definite shape or volume; particles are far apart and move rapidly.

Changes of State

• Melting: Solid to liquid

• Freezing: Liquid to solid

• Vaporization: Liquid to gas

• Condensation: Gas to liquid

• Sublimation: Solid to gas

• Deposition: Gas to solid

Temperature Scales

• Celsius (°C): Water freezes at 0°C and boils at 100°C.

• Kelvin (K): Absolute temperature scale; 0 K is absolute zero.

• Fahrenheit (°F): Water freezes at 32°F and boils at 212°F.

Conversion formulas:

• $K = ^\circ C + 273.15$

• $^\circ F = (1.8 \times ^\circ C) + 32$

• $^\circ C = \frac{^\circ F - 32}{1.8}$

Summary Table: States of Matter

State	Shape	Volume	Particle Arrangement	Particle Motion
Solid	Definite	Definite	Closely packed	Vibrate slowly
Liquid	Indefinite	Definite	Close, but mobile	Move moderately
Gas	Indefinite	Indefinite	Far apart	Move rapidly

Practice and Application

• Practice writing Lewis dot symbols for main group elements.

• Predict the charge of ions based on group number.

• Write formulas and names for ionic compounds, including those with transition metals.

• Classify substances as solid, liquid, or gas based on their properties.

• Convert between Celsius, Kelvin, and Fahrenheit temperature scales using the provided formulas.

Additional info: Some tables and examples were inferred and expanded for clarity and completeness. The notes are structured to provide a comprehensive overview suitable for GOB Chemistry students preparing for exams.