Essential Question: How do atoms of the same element differ?

Slides:

Advertisements

Similar presentations

4.3: HOW ATOMS DIFFER ATOMIC NUMBER

Advertisements

Subatomic Particles Atomic Number | Isotopes | Ions.

Atomic Structure Nucleus – contains protons and neutrons

Chapter 3 Atoms and Elements

Atomic Mass & Number Isotopes The Periodic Table.

Essential Question: How do atoms of the same element differ?

 Protons, neutrons, electrons too  Make up the atoms all around you!

Chapter 4 Lecture Basic Chemistry Fourth Edition Chapter 4 Atoms and Elements 4.5 Isotopes and Atomic Mass Learning Goal Give the number of protons, electrons,

Components of the Atom Nucleus: Nuclear Forces:

General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.1 Chapter 3 Atoms and Elements 3.5 Isotopes and Atomic Mass.

Atomic Structure and the Periodic Table

Chapter 4 Atoms and Elements

Counting Atoms.

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.

Isotopes Atoms of the same element that different mass numbers

How Atoms Differ.

The Structure of the Atom. Modern Concept of Atomic Theory 1.Atom consists of a tiny nucleus 2.Electrons move in an area directly surrounding the nucleus.

Chapter 3 Atoms and Elements 3.5 Atomic Number and Mass Number 1.

Chapter 3 Atoms and Elements 3.5 Isotopes and Atomic Mass 1 Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition.

THE ATOM Counting. The Atom  Objectives Explain what isotopes are Define atomic number and mass number, and describe how they apply to isotopes Given.

Unit 2 Review - Section 1 Atomic Structure and Mass.

 Determines the element  Number of protons CANNOT change for an element  Common charge notation is +1  Mass (g) = x  Mass (amu)=

How atoms differ. Mass Number The sum of the protons and neutrons BUT…Why is it not an even number??

Masses of Atoms Chapter 19-2 Pages

Chapter 4 Atoms and Elements

 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.

Atomic Structure Unit 3.

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

Do Now: If a student’s grade is weighted per the table below, what would their grade be? WeightAverage Tests50%80 Classwork30%95 Homework20%85.

 The weighted average of its naturally occurring isotopes. Chemical Name Atomic # Chemical Symbol Atomic Mass (Average Atomic Mass)

Atoms & Their Structure Chapter 2 Section 1 Part 3.

Average Atomic Mass. Relative Atomic Masses  Masses of atoms (in grams) are very small, so for convenience we use relative masses.  Carbon-12 is our.

Chemistry Chapter 4 Notes #2 (sec. 3). Periodic Table  All atoms are composed of smaller particles including equal numbers of protons (+) and electrons.

Atomic Number & Atomic Mass

Isotopes. The Nucleus  The number of protons in the nucleus of an atom is unique to each type of element  BUT, the nuclei of the same type of element.

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

General, Organic, and Biological Chemistry

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

LEARNING ABOUT ATOMS BY READING THE PERIODIC TABLE.

 Determines the element  Number of protons CANNOT change for an element  Common charge notation is +1  Mass (g) = x  Mass (amu)=

Unit 3: The Atom. Atoms All matter is made of very tiny particles All matter is made of very tiny particles These particles have the same properties as.

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.

Distinguishing among Atoms

Isotopic Abundance Pages Thinking question Why are there decimal places for atomic masses on the periodic table if protons and neutrons have amu.

 The basic unit of an element that can retain the properties of that element in a chemical reaction.

 Atom – the smallest particle of an element that retains the properties of that element.  When we say “small,” we mean “SMALL!”  A typical copper penny.

Unit 3 Atomic Structure and Periodicity. Dalton’s Atomic Theory 1.All matter is composed of _____________. 2. Atoms of the same element are _______________.

1 The Atom Atomic Number and Mass Number Isotopes.

4.5 Isotopes and Atomic Mass

Isotopes and Atomic Mass

Masses of Atoms.

How Atoms Differ.

Atomic Structure Concepts.

Chapter 4 Atoms and Elements

Learning Check Naturally occurring carbon consists of three isotopes: Carbon-13, Carbon-14, and Carbon-15. State the number of protons, neutrons, and.

Chapter 3 Objectives Explain what isotopes are.

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

Atomic Structure Chemistry.

Do First Actions: Get the 4 sheets: Atomic Structure Interactive, Calculating Protons, Neutrons, and Electrons Sheet, Bohr Model worksheet and It’s Natural.

Atomic Structure Chemistry.

ATOMIC STRUCTURE Chapter 4.

Distinguishing Among Atoms

Atomic # Atomic Mass #protons #neutrons Nitrogen-15 Oxygen-18

Section 2: Masses of Atoms

Presentation transcript:

Essential Question: How do atoms of the same element differ? Isotopes Essential Question: How do atoms of the same element differ?

ISOTOPES What are they? Isotopes are atoms of the same element that have the same number of protons but a different number of neutrons. All elements consist of naturally occurring isotopes.

How are isotopes of an element similar? How are they different? The isotopes of an element have Different Physical Properties (different mass and different number of neutrons) Identical Chemical Properties (this is because they have the same numbers of protons and electrons and subatomic particles are responsible for chemical behavior)

NUCLEAR SYMBOLS Nuclear symbols are used to represent specific isotopes. To write a nuclear symbol, the symbol of the element is written first, the mass number is written as a superscript to the left of the symbol and the atomic number is written as a subscript to the left. Study the illustration below. Li-7 isotope

WRITING ISOTOPES You can also use the mass number and the name of the element to designate the atom or isotope. For example, two isotopes of carbon are carbon-12 and carbon-13. The symbols for these two isotopes would be: C 12 6 C 13 6

The mass number refers to the total number of protons and neutrons in a specific nucleus of an atom. The atomic number always refers to the total number of protons in an atom. To determine the number of neutrons in a specific isotope, subtract the atomic number from the mass number. Study the formula below. Mass Number (neutrons + protons) - Atomic Number (number of protons) (number of neutrons)

Boron consists of two isotopes, B-10 and B-11 Boron consists of two isotopes, B-10 and B-11. Determine the number of neutrons in each of the isotopes. From the periodic table, write the symbol and atomic number for Boron. Determine the number of neutrons by subtracting the atomic number from the mass number. B-10: 10 – 5 = 5 neutrons B-11: 11 – 5 = 6 neutrons

Mass Number and Atomic Mass To identify isotopes, the mass number is added after the element’s name. Ex: potassium-39 potassium-40 Atomic mass of an element is the weighted average mass of the isotopes of that element It’s calculated by summing the products of each isotope’s percent abundance times its atomic mass. Refer to pg 103 in the text for the example (6.015 amu)(0.0750) + (7.016amu)(0.925) = 6.941amu

Nuclear Symbol Complete based on the following information: 29 protons, mass 65 Barium - 138 17 protons, mass 36 Tin - 120 16 protons, mass 30