2. Atoms & Elements

Atomic Theory

Development of Atomic Theory: An Introduction

A chemical reaction rearranges the grouping of atoms.

Atoms are composed of protons, neutrons, and electrons.

Atoms of a given element are chemical and physically identical.

Atoms of different elements combine in simple, whole number ratios to form compounds.

Matter is composed of atoms that are unable to divided any further.

Which of the following is NOT a component of Dalton’s Atomic Theory?

A chemist finds that 30.82 g of nitrogen will react with 17.60, 
35.20, 70.40, or 88.00 g of oxygen to form four different 
compounds. (b) How do the numbers in 
part (a) support Dalton’s atomic theory?

Dalton used the lightest element as his standard for atomic mass. What is this element?

How does Dalton’s atomic theory account for the law of mass conservation and the law of definite proportions?

Atomic Theory of Matter

Week1 Chemistry Atomic Theory Timeline Lesson 2.1a SDS

Which statements are consistent with Dalton’s atomic theory as it was originally stated? Why?
a. Sulfur and oxygen atoms have the same mass.
b. All cobalt atoms are identical.
c. Potassium and chlorine atoms combine in a 1:1 ratio to form potassium chloride.
d. Lead atoms can be converted into gold.

Dalton’s Atomic Theory | Don't Memorise

Which statements are inconsistent with Dalton’s atomic theory as it was originally stated? Why? 
a. All carbon atoms are identical. 
b. An oxygen atom combines with 1.5 hydrogen atoms to form a water molecule. 
c. Two oxygen atoms combine with a carbon atom to form a carbon dioxide molecule. 
d. The formation of a compound often involves the destruction of one or more atoms.

Lesson 6 - Atomic Theory Of Matter, Part 1 (Chemistry Tutor)

History of Atomic Theory

Atomic theory | Matter | Physics | FuseSchool

The 2,400-year search for the atom - Theresa Doud

The History of Atomic Chemistry: Crash Course Chemistry #37

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed
into its elements, yielding 0.273 g of carbon and 0.727 g of
oxygen. If a sample of a different compound decomposes into 0.429 g of
carbon and 0.571 g of oxygen, what is its ratio of the mass of
O to C? (c) According to Dalton’s atomic theory, what is the
empirical formula of the second compound?

Atomic Theory Example 1

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1. Intro to General Chemistry

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Millikan Oil Drop Experiment

The Oil Drop Experiment helped with determining the fundamental charge of the electron.&nbsp;

Ions

Ions represent elements that possess either a positive charge or a negative charge.&nbsp;

Periodic Table: Charges

Elements lose or gain electrons to have the ideal number of outer shell electrons like the noble gases.&nbsp;

Law of Definite Proportions

"Different samples of a pure chemical compound always contain the same proportions of elements by mass."

Periodic Table: Classifications

The Periodic Table contains 3 Major Classifications when describing its elements

Isotopes

Isotopes are atoms of an element that have the same atomic number, but different mass number.&nbsp;

The Atom

The atom represents the basic functional unit in chemistry

Mole Concept

The Mole Concept involves the interconversions between different unit amounts of a substance.

Periodic Table: Representative Elements & Transition Metals

The Groups of the Periodic Table can be broken down into the Representative Elements and Transition Metals

John Dalton, one of the "Fathers of Chemistry"is credited with modernizing the Atomic Theory.

Subatomic Particles

The atom is composed of 3 subatomic particles:neutrons, protons, and electrons.

Periodic Table: Elemental Forms

The elements of the Periodic Table exist in different elemental forms in the natural world

Periodic Table: Phases

Under standard conditions of temperature and pressure, the elements can exist as solids, liquids or gases

Atomic Mass

The atomic mass of an element includes the masses of all 3 subatomic particles of neutrons, protons and electrons.&nbsp;

Periodic Table: Group Names

The Periodic Table can be further classified into Periods and Groups.&nbsp;

Law of Conservation of Mass

"In a chemical reaction, no matter is created or destroyed, but instead changes form."

Calculating Molar Mass

Molar Mass is a physical property that represents the mass of a substance divided by the amount of that substance.

Rutherford Gold Foil Experiment

The Gold Foil Experiment helped with the discovery of the positively charged nucleus.

Law of Multiple Proportions

“When 2 elements (A &amp; B) form different compounds, the mass of Element B that combine with 1 g of A are a ratio of whole numbers."

Periodic Table: Element Symbols

The Element Symbols of the Periodic Table represent the abbreviated form of an element

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