Explain The Law Of Conservation Of Mass And Law Of Multiple Proportions Using Examples Accordingly Of What Is And Is Not Possible Explain The Evidence (And Associated Experiments) That Lead Us To Adopt The Nuclear Model Of The Atom And Reject The Plum Pudding Model Of The Atom Describe The Generic Structure Of An Atom Calculate The Correct Number Of Subatomic Particles For Any Isotope Of Any Element Calculate The Atomic Mass Of An Element From Information Of Its Isotopes (Mass And Abundance) And Visa Versa Identify The Parts Of The Periodic Table And Explain Why The Periodic Table Has The Form That It Does Explain The Relationship Between Atoms And Ions Name A Substance From Its Formula And Derive Its Formula From Its Name

Substance from Formula:

• Formula: H₂O

• Name: Water

Deriving Formula from Name:

• Name: Sodium Chloride

• Formula: NaCl

Law of Conservation of Mass

• Definition: Mass is neither created nor destroyed in a chemical reaction.

• Example: In a closed system, if 10g of reactants yield 10g of products, mass is conserved.

Law of Multiple Proportions

• Definition: When two elements form different compounds, the mass ratios of the elements are simple whole numbers.

• Example: CO (carbon monoxide) and CO₂ (carbon dioxide) have a mass ratio of 1:2 for oxygen.

Evidence for Nuclear Model

• Experiments: Rutherford's gold foil experiment showed that atoms have a dense nucleus, rejecting the plum pudding model which suggested a diffuse distribution of charge.

Generic Structure of an Atom

• Components: Nucleus (protons and neutrons) surrounded by electrons in orbitals.

Subatomic Particles Calculation

• Example: Carbon-14 (C-14) has 6 protons, 8 neutrons, and 6 electrons.

Atomic Mass Calculation

• Formula: Atomic mass = (mass of isotope₁ × abundance₁) + (mass of isotope₂ × abundance₂).

Periodic Table Structure

• Parts: Organized by increasing atomic number, groups (columns) share chemical properties, periods (rows) indicate energy levels.

Relationship Between Atoms and Ions

• Definition: Atoms become ions by gaining or losing electrons, resulting in a charge.

Naming and Deriving Substances

• Example: NaCl is sodium chloride; derived from sodium (Na) and chlorine (Cl).