Chemistry Review Atomic Theory and Atomic Structure Who

  • Slides: 32
Download presentation
Chemistry Review Atomic Theory and Atomic Structure

Chemistry Review Atomic Theory and Atomic Structure

Who am I?

Who am I?

Responsible for naming the atom 1. 2. 3. 4. Dalton Bohr Rutherford Democritus

Responsible for naming the atom 1. 2. 3. 4. Dalton Bohr Rutherford Democritus

Who am I?

Who am I?

I proposed the atomic theory. 1. 2. 3. 4. 5. Bohr Rutherford Chadwick Dalton

I proposed the atomic theory. 1. 2. 3. 4. 5. Bohr Rutherford Chadwick Dalton Democritus

How was my atomic theory incorrect? All elements are composed of atoms which are

How was my atomic theory incorrect? All elements are composed of atoms which are indivisible. 2. Atoms of the same element are alike. 3. Compounds form by joining 2 or more elements. 1.

Whose model is this?

Whose model is this?

The previous model showed positive and negative charges mixed like “Plum Pudding” 1. 2.

The previous model showed positive and negative charges mixed like “Plum Pudding” 1. 2. 3. 4. Bohr Dalton Thomson Rutherford

Who am I and here is my model

Who am I and here is my model

Discovered the nucleus had a positive charge with electrons outside of it. 1. 2.

Discovered the nucleus had a positive charge with electrons outside of it. 1. 2. 3. 4. Bohr Dalton Rutherford Thomson

Rutherford Gold Foil Experiment The reflected alpha particles bounced off of the positively charged

Rutherford Gold Foil Experiment The reflected alpha particles bounced off of the positively charged nucleus – which proved the existence of the nucleus. True or False? True – alpha particles are positive The reflected alpha particles bounced off of the atoms in the gold foil – which proved the existence of atoms. True or False? False

Rutherford Gold Foil Experiment Most of the alpha particles went straight through the gold

Rutherford Gold Foil Experiment Most of the alpha particles went straight through the gold foil undeflected – which proved that the positive charge was spread out evenly through the atom. True or False. Positive would reflect positive.

Who am I ?

Who am I ?

My contribution to the atomic theory development was Nothing, I was a loser. Discovered

My contribution to the atomic theory development was Nothing, I was a loser. Discovered protons. Placed electrons in specific energy levels. 4. Discovered neutrons. 1. 2. 3.

Who am I ?

Who am I ?

Who am I and what did I do? Rutherford and discovered protons and nucleus.

Who am I and what did I do? Rutherford and discovered protons and nucleus. 2. Thompson and discovered electrons. 3. Chadwick, and discovered neutrons. 1.

Why were the neutrons so difficult to detect? 1. 2. 3. Because they are

Why were the neutrons so difficult to detect? 1. 2. 3. Because they are so massive. Because they have no charge. Because they have numerous charges.

Subatomic Particles Particle Symbol Charge Electron e- - Proton p+ + Neutron n neutral

Subatomic Particles Particle Symbol Charge Electron e- - Proton p+ + Neutron n neutral Relative Mass 0 1 1

State the number of protons for Nitrogen 1. 2. 3. 5 protons 7 protons

State the number of protons for Nitrogen 1. 2. 3. 5 protons 7 protons 14 protons

State the number of protons for Sulfur 1. 2. 3. 32 protons 16 protons

State the number of protons for Sulfur 1. 2. 3. 32 protons 16 protons

State the number of protons for Barium 1. 2. 3. 137 protons 81 protons

State the number of protons for Barium 1. 2. 3. 137 protons 81 protons 56 protons

Number of Electrons l. An atom is neutral l. The net charge is zero

Number of Electrons l. An atom is neutral l. The net charge is zero l. Number of protons = Number of electrons l. Atomic number = Number of electrons

Ions – charged atoms If an ion gains an electron it becomes _______ charged

Ions – charged atoms If an ion gains an electron it becomes _______ charged and is called an _______. Answer: negatively anion

Ions: charged atoms If an ion loses an electron , it becomes ______ charged,

Ions: charged atoms If an ion loses an electron , it becomes ______ charged, and is called a _______. Answer: positively, cation

An atom of zinc has a mass number of 65. Number of protons in

An atom of zinc has a mass number of 65. Number of protons in zinc are 1. 2. 3. 4. 30 35 65 125

The number of neutrons in zinc are 1. 2. 3. 4. 30 35 65

The number of neutrons in zinc are 1. 2. 3. 4. 30 35 65 125

What is the mass number of a zinc isotope with 37 neutrons? 1. 2.

What is the mass number of a zinc isotope with 37 neutrons? 1. 2. 3. 4. 37 65 67 125

An atom has 14 protons and 20 neutrons. Its atomic number is 1. 2.

An atom has 14 protons and 20 neutrons. Its atomic number is 1. 2. 3. 4. 14 16 34 201

An atom has 14 protons and 20 neutrons. Its mass number is 1. 2.

An atom has 14 protons and 20 neutrons. Its mass number is 1. 2. 3. 4. 14 16 34 8

An atoms has 14 protons and 20 neutrons. The element is 1. 2. 3.

An atoms has 14 protons and 20 neutrons. The element is 1. 2. 3. 4. Si Ca Se Lol

If an element has 12 protons and 12 neutrons, how many electrons are found

If an element has 12 protons and 12 neutrons, how many electrons are found in the nucleus? A. 12 B. 24 C. Only the ones with lots of energy. D. No electrons are found in nucleus.

Ions 37 Cl -1 17 How many protons? How many neutrons? How many electrons?

Ions 37 Cl -1 17 How many protons? How many neutrons? How many electrons? Anion or Cation?

IB Chemistry ATOMIC THEORY Atomic Structure Atomic StructureIB Chemistry ATOMIC THEORY Atomic Structure Atomic Structure
Atomic Structure Modern Atomic Theory Modern Atomic TheoryAtomic Structure Modern Atomic Theory Modern Atomic Theory
Atomic Structure Basic Atomic Structure Basic Atomic StructureAtomic Structure Basic Atomic Structure Basic Atomic Structure
Atomic and Nuclear Physics Atomic structure Atomic StructureAtomic and Nuclear Physics Atomic structure Atomic Structure
Atomic Theory Chemistry Early Atomic Theories first theoryAtomic Theory Chemistry Early Atomic Theories first theory
ATOMIC STRUCTURE Chemistry 11 Atomic Theory 2 SUBATOMICATOMIC STRUCTURE Chemistry 11 Atomic Theory 2 SUBATOMIC
IB Chemistry TOPIC 10 ATOMIC THEORY Atomic StructureIB Chemistry TOPIC 10 ATOMIC THEORY Atomic Structure
ATOMIC STRUCTURE AS Chemistry Basic Atomic Structure HyATOMIC STRUCTURE AS Chemistry Basic Atomic Structure Hy
Atomic Theory Structure Atomic Theory Developed over 2000Atomic Theory Structure Atomic Theory Developed over 2000
Unit 3 Atomic Theory Structure Modern Atomic TheoryUnit 3 Atomic Theory Structure Modern Atomic Theory
Atomic structure Atomic Structure The structure of theAtomic structure Atomic Structure The structure of the
Atomic structure Atomic Structure The structure of theAtomic structure Atomic Structure The structure of the
ATOMIC THEORY REVIEW VOCABULARY AND ATOMIC STRUCTURE UNITATOMIC THEORY REVIEW VOCABULARY AND ATOMIC STRUCTURE UNIT
Atomic Theory Review Basic Atomic Structure A LookAtomic Theory Review Basic Atomic Structure A Look
Atomic Theory Review Basic Atomic Structure A LookAtomic Theory Review Basic Atomic Structure A Look
Atomic Structure Review Isotopes Atomic Structure n TheAtomic Structure Review Isotopes Atomic Structure n The
Matter and Atomic Structure Matter and Atomic StructureMatter and Atomic Structure Matter and Atomic Structure
MATTER AND ATOMIC STRUCTURE MATTER AND ATOMIC STRUCTUREMATTER AND ATOMIC STRUCTURE MATTER AND ATOMIC STRUCTURE
Structure of Matter Atomic Macro Atomic Macro AtomicStructure of Matter Atomic Macro Atomic Macro Atomic
Atomic Structure Calculating Average Atomic Mass Average AtomicAtomic Structure Calculating Average Atomic Mass Average Atomic
Atomic Structure Atomic Notation Atomic Notation represents theAtomic Structure Atomic Notation Atomic Notation represents the
Structure Structure Structure 1 2 End Structure StructureStructure Structure Structure 1 2 End Structure Structure
Atoms and Atomic Theory Atomic Theory As earlyAtoms and Atomic Theory Atomic Theory As early
Atoms and Atomic Theory Atomic Theory As earlyAtoms and Atomic Theory Atomic Theory As early