Atomic Number, Mass Number, Atomic Mass and Isotopes

Slides:

Advertisements

Similar presentations

Atomic Number, Mass Number, Atomic Mass and Isotopes Mrs. Coyle Chemistry.

Advertisements

Atomic Structure Nucleus – contains protons and neutrons

Atomic Mass & Number Isotopes The Periodic Table.

Mass Number Atomic Number equals the # of... NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE ATOM.

How Atoms Differ.

Atomic Number, Mass Number, Atomic Mass and Isotopes

Do Now (In your Tracker)  Read the article and underline any words that you do not know. Answer the following questions: 1. What is the main idea of the.

Isotopes. Isotopes are atoms that have the same number of protons but different numbers of neutrons Most elements in the first two rows of the periodic.

 Atomic Number- the number of protons in the nucleus of an atom of that element  Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.

Mass Spectrometer. Atomic Number Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. Element# of protonsAtomic.

Atomic Structure.  Atomic number – the number of protons in the nucleus of an atom ( ID of element )  Mass number– sum of protons and neutrons in an.

Section 4.3 How atoms differ. Atomic Number Represents three things in a neutral atom: 1. What element it is 2. The number of protons in each atom 3.

Atomic Structure The Periodic Table, Isotopes, and Average Atomic Mass.

Atoms / Elements Different number of protons Protons found in nucleus # of protons = atomic number Since atom is electrically neutral: #protons = # electrons.

Rutherford’s Atom/Past Electrons orbit nucleus similar as planets to the sun Atom of the Present Electrons orbit nucleus in the form of clouds.

Isotopes. Let’s Review ProtonsNeutronsElectrons Charge +1 0 Mass 1 amu 0 Location nucleus Electron cloud.

Proton A positively charged subatomic particle (found in the nucleus). A subatomic particle with no charge (found inside the nucleus). Neutron.

Atomic Structure What are atoms made of? How are atoms put together? What are Elements? Isotopes?

Parts of the Atom: Properties  Protons: –Positive charge –Located in nucleus –Mass = 1 amu (Atomic Mass Unit)  Neutrons –No charge (neutral) –Inside.

4.3 Atomic #, Mass #, Atomic Mass & Isotopes. Atomic Number  What are the 3 subatomic particles?  Which of the subatomic particles identifies an element?

Isotopes vs. Ions.

Atomic Structure Concepts.

Atomic Structure Subatomic Particles C. Johannesson.

4.2 – NOTES The Mass of the Atom

4.2 -Atomic Structure Theory

Atomic Structure Atoms are made of 3 subatomic particles:

ELEMENTS, IONS AND ISOTOPES

Atoms / Elements •Different number of protons

Atomic Structure.

Atomic Structure.

Subatomic Particles Subatomic particles - 3 important to chemistry

Unit 2: Atomic Theory & Structure

Unit 2: Atomic Theory & Structure

The atom and Isotopes.

Basic Atomic Structure

Subatomic Particles.

Atomic Symbols protons + neutrons = mass # atomic # = protons.

Mr. Anthony Gates AP Chemistry Unit 9

Distinguishing Between Atoms

Atomic Variation.

H H H Isotopes element: same or different mass:

Structure of The Atom Not the Adam.

H H H Isotopes element: same or different mass:

Atomic Structure Chemistry.

Foldables: Atoms Terms.

Subatomic Particles.

Elements, Isotopes and More

Ch. 3 Atoms 3.3 Counting Atoms.

Atomic Structure Chemistry.

Atomic Symbols protons + neutrons = mass # atomic # = protons.

Ch. 3 - Atomic Structure II. Masses of Atoms (p.75-80) Mass Number

Warm Up 1.What did Rutherford’s scattering experiment show? Need to list 2 important findings. 2. What did Thomson discover? Describe the atomic model.

Chemistry Unit: Chapter 3

Atomic Symbols = = mass # atomic # protons + neutrons protons

Atomic Symbols protons + neutrons = mass # atomic # = protons.

Chapter 4 – The Structure of the Atom

Atomic Structure Nucleons Atomic Number

Ch. 4 - Atomic Structure II. Masses of Atoms Mass Number Isotopes

Atomic Structure Nucleus Protons Neutrons Electrons.

ARE ALL ATOMS OF THE SAME ELEMENT IDENTICAL?

Structure of an Atom What is an ATOM??? Pg

Subatomic Particles.

Example Example 1: The atom of an element has a mass number of 214 and an atomic number of 82. a) How many protons and neutrons does it have? The number.

Atomic Particles Particle Charge Mass (kg) Location Electron -1

Presentation transcript:

Atomic Number, Mass Number, Atomic Mass and Isotopes Ms. McCallum Chemistry

Atomic Number (Z): is the number of protons in the nucleus of the atom. Z=#p

The number of protons (atomic number) determine the identity of an element.

Atoms have no overall electrical charge so, an atom must have as many electrons as there are protons in its nucleus.

The atomic number of an element also equals the number of electrons in a neutral atom of that element.

Ex: Sodium What is the atomic number of Sodium? How many protons does sodium have? How many electrons does sodium have?

Mass Number (A): The sum of the protons and neutrons in the nucleus. A=#p + #n

Notation

Other ways to write elements: 36 17Cl Cl-36 Mass Number Mass Number Atomic Number

Nucleons: protons and neutrons

Isotopes of an element have different mass numbers because they have different numbers of neutrons, but they have the same atomic number.

Example: Isotopes of Carbon and Hydrogen protium deuterium tritium H H H Isotopes of Hydrogen Isotopes of Carbon

is a unit used to compare Atomic Mass Unit is a unit used to compare the masses of atoms and has the symbol u or amu.

is approximately equal to 1 amu or u is approximately equal to the mass of a single proton or neutron.

Carbon-12 Chemists have defined the carbon-12 atom as having a mass of 12 atomic mass units.

1 u = 1/12 the mass of a Carbon-12 atom.

Atomic Mass is the weighted average mass of all the naturally occurring isotopes of that element.