Isotopes. Subatomic Particles # protons = atomic number Carbon - atomic number 6; # of protons 6 # electrons (neutral atom) = # protons Carbon - # protons.

Slides:

Advertisements

Similar presentations

Atomic Structure Nucleus – contains protons and neutrons

Advertisements

ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons A Z X A = mass number (the total number of protons.

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

Subatomic Particles. 1. Subatomic Particles ParticleSymbol (table O) ChargeMass (amu) Location Electrons e 0 e -1 0 β -1 Negative (-1) 1/1872 amu 0 amu.

Isotopes and Mass Number. Atomic Number The number of protons in each atom identifies it as an atom of a particular element Each atom has a unique number.

Subatomic Particles  Protons and electrons are the only particles that have a charge.  Protons and neutrons have essentially the same mass.  The mass.

Dalton was proved incorrect and his theory was modified

Atomic Structure I. Subatomic Particles.

Distinguishing Between Atoms

Chapter 4 Atomic Structure 4.3 Distinguishing Among Atoms

Isotopes Atoms of the same element that different mass numbers

Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Just as there are many types of dogs, atoms come in different varieties too.

GHSGT Comprehensive Review Day 1 Structure and Properties of Atoms.

4.3 Distinguishing Among Atoms > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 4 Atomic Structure 4.1 Defining.

How Atoms Differ.

Chapter 4 Atomic Structure 4.3 Distinguishing Among Atoms

Structure of an Atom. What are the fundamental particles of the atom? Proton: Particle with positive electrical charge (+1). Electron: Particle with negative.

Chapter 4 Atomic Structure 4.3 Distinguishing Among Atoms

Periodic Table Name Symbol Atomic Number Weight Electro-negativity

Chapter 4 Atomic Structure 4.3 Distinguishing Among Atoms

Unit 2 Review - Section 1 Atomic Structure and Mass.

+ ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons.

Isotopes  Atoms with the same number of protons but different numbers of neutrons  Ex) Carbon 12 vs. Carbon 14  These atoms have a different mass 

Isotopic Abundance SCH 3U. Atomic Mass The mass of an atom (protons, neutrons, electrons) Relative Atomic Mass: An element’s atomic mass relative to the.

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.

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.

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.

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

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

Isotopes and Mass Number. Isotope Atoms of the same element with: Same number of protons BUT Different number of neutrons ELEMENT IS TO ISOTOPE AS DOG.

4.3 Distinguishing Among Atoms > 1 9/22/15 ll ork 1: Draw an atom based on your current understanding of subatomic particles. Label each part. 2: Why must.

Isotopes & Ions 4.7; Subatomic Particles Remember Dalton?  Remember Dalton’s atomic theory?  “All atoms of a given element are identical”. 

Atomic Number & Mass Number All atoms consist of protons and electrons- most also have neutrons Protons & neutrons- in the small dense nucleus- similar.

4.3 Distinguishing Among Atoms > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 4 Atomic Structure 4.1 Defining.

Isotopes and abundance. The relative atomic mass scale is now based on an isotope of carbon, carbon-12, which is given the value of amu.

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

1 The Atom Atomic Number and Mass Number Isotopes.

Same Element Different Atom- Isotopes All atoms of a particular element are not exactly alike. Some elements have atoms with different masses (isotopes)

4.3 Distinguishing Among Atoms > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 4 Atomic Structure 4.1 Defining.

Isotopes are atoms of the same element that have a different number of neutrons For example, Hydrogen has 3 isotopes: Protium (0 neutrons) Deuterium (1.

Chapter 4 Atomic Structure 4.1 Defining the Atom

Isotopes and Atomic Mass

Atomic Structure Current Atomic model

Atomic Structure.

Calculating Average Mass

Unit 3 – Atoms, Ions, Isotopes

Atoms / Elements •Different number of protons

Chapter 4 Atoms and Elements

Atomic Structure.

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

The atom and Isotopes.

Subatomic Particles.

ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons A Z X A = mass number (the total number of protons.

Lesson 13: Subatomic Heavyweights

Chapter 4 Atomic Structure 4.1 Defining the Atom

Atomic Structure.

Subatomic Particles.

Ch. 3 Atoms 3.3 Counting Atoms.

How Atoms Differ Chp 4.

Chapter 4 Atomic Structure 4.1 Defining the Atom

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

Chapter 4 Atomic Structure 4.1 Defining the Atom

Element properties & isotopes

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

Atomic Structure Nucleons Atomic Number

Atomic Number, Mass Number, Atomic Mass and Isotopes

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

ARE ALL ATOMS OF THE SAME ELEMENT IDENTICAL?

Subatomic Particles.

Presentation transcript:

Isotopes

Subatomic Particles # protons = atomic number Carbon - atomic number 6; # of protons 6 # electrons (neutral atom) = # protons Carbon - # protons 6 = # electrons 6 # neutrons = mass number – atomic number Carbon-12 6 neutrons = 12 (mass number) – 6 (atomic number)

ATOMS OF THE 1 ST TEN ATOMS NAMESYMBOL ATOMIC # p+p+p+p+ n0n0n0n0 MASS # e-e-e-e- HydrogenH11011 HeliumHe22242 LithiumLi33473 BerylliumBe44594 BoronB CarbonC NitrogenN OxygenO FluorineF NeonNe

Isotope: two or more atoms having the same number of protons but different numbers of neutrons or Na-23 or Na-24

Every Cl atom has 17 protons, w/o exception, but not every Cl atom has 18 neutrons. – Atoms with the same # of protons but contain different #s of neutrons are called isotopes. Since isotopes of an element have different #s of neutrons they have different masses

Isotopes are chemically alike because they have identical numbers of protons and electrons – It’s the electrons and protons that are responsible for chemical behavior Isotopes can be noted using hyphen notation (Cl-35 vs. Cl-37) or (Chlorine – 35 vs. Chlorine – 37) – element symbol hyphen mass number – element name hyphen mass number

Hydrogen Isotopes Nuclide #p+ #n 0 # e- at. # mass number (#p+ and #n0) Protium (1 + 0) Deuterium (1 + 1) Tritium (1 + 2)

9 H 3 1 H 2 1 H 1 1 Hydrogen Isotopes

Write the hyphen notations for the following:

Average Atomic Mass This is the mass that is on the periodic table. It is a weighted average of the masses of all the isotopes of a particular element. Atomic mass = (mass isotope 1)(% abundance) + (mass isotope 2)(% abundance) This is what is located on the periodic table

Practice 1.Naturally occurring chlorine is 75.53% chlorine- 35 and 24.47% chlorine-37. What is the average atomic mass? Ans. (0.7553)(35) + (0.2447)(37) = 1.The element Neon consists of three isotopes with masses 19.99, 20.99, and amus. These three isotopes are present in nature to the extent of 90.51%, 0.27%, and 9.22% respectively. Calculate the atomic mass of neon.

Isotopes of Neon Isotopes% in Nature Atomic Number Atomic Mass (amu) 1 atom Mass Number Average Atomic Mass (amu) Ne % amu amu Ne % amu 21 Ne % amu 22

3.The element silver exists in nature as two isotopes Ag-107 and Ag-109. The accepted atomic mass of silver is amu. What isotope is more abundant?

4.Calculate the average atomic mass of an element given the following information: Nitrogen-15 is 30% abundant Nitrogen-13 is 20% abundant Nitrogen-14 is 50% abundant