Chapter 18 Lesson 2 Masses of Atoms

Slides:

Advertisements

Similar presentations

4.3: HOW ATOMS DIFFER ATOMIC NUMBER

Advertisements

17.2 Masses of Atoms. Atomic Mass The nucleus contains most of the mass of the atom bc P and N are far more massive than E. P & N are about the same size.

Atomic Structure Nucleus – contains protons and neutrons

Atomic Mass & Number Isotopes The Periodic Table.

Atomic Structure and the Periodic Table

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

Atomic Structure I. Subatomic Particles.

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

Section 2: Masses of Atoms

Chapter 18 Lesson 2 Masses of Atoms

Atomic Mass Notes 5 Chapter 17-2.

Masses of Atoms Chapter 19-2 Pages

Chapter 4.3 Distinguishing Among Atoms

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

Atomic Mass. Masses in amu Only carbon-12 has an atomic mass exactly equal to its mass # One atomic mass unit (amu) is defined as 1/12 the mass of a carbon-12.

Atoms & Their Structure Chapter 2 Section 1 Part 3.

I. Subatomic Particles (p ). ParticleSymbolLocationChargeRelative Mass (amu) Actual Mass (g) electron proton neutron e-e- p+p+ n0n0 Electron.

Unit 3: Atomic Structure. A. Subatomic Particles Most of the atom’s mass (Mass Number) NUCLEUS ELECTRON CLOUD PROTONS NEUTRONS ELECTRONS POSITIVE CHARGE.

How Atoms Differ. a. Properties of Subatomic Particles ParticleSymbolLocationRelative Charge Relative mass Actual mass (g) Electron Proton Neutron.

Note: When doing calculations never clear your calculator.

Atomic Mass. Atomic mass Most of the mass of an atom is in the nucleus. Most of the mass of an atom is in the nucleus. The nucleus is where all of the.

Chapter 3 Isotopes Part II. Atoms Nucleus is center core. Nucleus is center core. Nucleus is made of Protons & Neutrons. Nucleus is made of Protons &

Masses of Atoms.

Section 2 Protons, neutrons, and electrons- how atoms differ

How Atoms Differ.

II. Masses of Atoms Mass Number

Calculating Average Mass

Atomic Structure Subatomic Particles C. Johannesson.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

The atom and Isotopes.

Isotopes and Calculating Atomic Mass

Ch Atomic Structure II. Masses of Atoms (p.30-31) Mass Number

Distinguishing Between Atoms

Atomic Structure.

Atomic Structure.

Isotopes - isotope: atoms of the same element that have different numbers of neutrons - Carbon, as found in nature, is a mixture of isotopes, including.

Structure of The Atom Not the Adam.

Atomic Structure Chemistry.

Section 1 Structure of the atom and cells on the periodic table

Foldables: Atoms Terms.

Mass of Individual Atoms

I. Atomic Structure II. Masses of Atoms Mass Number Isotopes Ion

Title: Atomic Properties

Intro to Atomic Structure

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

III. Masses of Atoms (p ) Atomic Mass Mass Number Isotopes

Atomic Structure Chemistry.

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

1. What are these two atoms of carbon called?

A. Structure of the Atom Chemical Symbols Subatomic Particles

AVERAGE ATOMIC MASS CALCULATIONS

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

Atomic Structure Nucleons Atomic Number

Atomic Number, Mass Number, Atomic Mass and Isotopes

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

III. Masses of Atoms Atomic Mass Mass Number Isotopes

I. Structure of the Atom Chemical Symbols Subatomic Particles

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

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

1. What are these two atoms of carbon called?

Introduction to Atomic Structure

The periodic table and the atom part 2

Section 2: Masses of Atoms

Counting Subatomic Particles

Presentation transcript:

Chapter 18 Lesson 2 Masses of Atoms

Atomic Mass The nucleus contains most of the mass of the atom because protons and neutrons are far more massive than electrons. The mass of a proton is about the same as that of a neutron—approximately

Atomic Mass The mass of each is approximately 1,836 times greater than the mass of the electron.

Atomic Mass The unit of measurement used for atomic particles is the atomic mass unit (amu). The mass of a proton or a neutron is almost equal to 1 amu. The atomic mass unit is defined as one-twelfth the mass of a carbon atom containing six protons and six neutrons.

Protons Identify the Element The number of protons tells you what type of atom you have and vice versa. For example, every carbon atom has six protons. Also, all atoms with six protons are carbon atoms. The number of protons in an atom is equal to a number called the atomic number.

Mass Number Sum of the protons and neutrons in the nucleus of an atom Always a whole number © Addison-Wesley Publishing Company, Inc.

Mass Number If you know the mass number and the atomic number of an atom, you can calculate the number of neutrons. number of neutrons = mass number – atomic number

Isotopes Mass # Atomic # Not all the atoms of an element have the same number of neutrons. Isotopes are atoms of the same element with different numbers of neutrons. Isotope symbol: Mass # Atomic # “Carbon-12”

Isotopes © Addison-Wesley Publishing Company, Inc.

Identifying Isotopes Models of two isotopes of boron are shown. Because the numbers of neutrons in the isotopes are different, the mass numbers are also different. You use the name of the element followed by the mass number of the isotope to identify each isotope: boron-10 and boron-11

Identifying Isotopes The average atomic mass of an element is the weighted-average mass of the mixture of its isotopes. For example, four out of five atoms of boron are boron-11, and one out of five is boron-10. To find the weighted-average or the average atomic mass of boron, you would solve the following equation: