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

Slides:

Advertisements

Similar presentations

4.3: HOW ATOMS DIFFER ATOMIC NUMBER

Advertisements

The Structure of the Atom The Building Block of Matter.

AIM: HOW TO CALCULATE THE AVERAGE ATOMIC MASS? DO NOW:1. WHAT ARE THE 3 SUBATOMIC PARTICLES OF AN ATOM? LIST THE THREE SUBATOMIC PARTICLES AND THEIR CHARGE.

Atomic Structure Nucleus – contains protons and neutrons

Chapter 3 Atoms and Elements

OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM

Atomic Mass & Number Isotopes The Periodic Table.

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

Bell work  1. Which subatomic particles reside in the nucleus?  2. If we are looking at Carbon-14, how many protons, electrons, and neutrons are present.

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,

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.

Dalton was proved incorrect and his theory was modified

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

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)=

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.

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.

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

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.

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.

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

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

Parts of the Atom … from Discovery to Reality. NUCLEUS PROTONS ✚ Positively charged particles Mass = 1 amu NEUTRONS No charge or neutral Mass = 1 amu.

Ch. 3-3a Distinguishing and Counting Atoms. POINT > Define Atomic Number POINT > Define Mass Number POINT > Describe and identify isotopes POINT > Determine.

Concept Check 2.1 Atomic Size

The Structure of the Atom The Building Block of Matter.

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

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)

Lesson 24: Isotopes An element can be identified by the # of protons it has # of neutrons can vary Neutrons add to the mass of the atom, but do not change.

4.5 Isotopes and Atomic Mass

Isotopes and Atomic Mass

How Atoms Differ.

Ch. 3-3a Distinguishing and Counting Atoms

II. Masses of Atoms Mass Number

Now you try! Helium – 4 Oxygen – 16 Magnesium – 26 Isotope

Warm Up Monday 1/25/16 1. What are atoms?

Atomic Structure Subatomic Particles C. Johannesson.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

Chapter 4 Atoms and Elements

Chapter 3 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.

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

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.

Section 3 Counting Atoms

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.

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

Element properties & isotopes

ATOMIC STRUCTURE Chapter 4.

Distinguishing Among Atoms

ATOM COMPOSITION The atom is mostly empty space

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

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

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

Presentation transcript:

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

What is an Isotope? 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 and artificially produced isotopes

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

How do we represent specific isotopes? Nuclear symbols are used to represent specific isotopes To write a nuclear symbol: 1.) the symbol of the element is written first 2.) the mass number is written as a superscript to the left of the symbol 3.) the atomic number is written as a subscript to the left. Study the illustration below Li-7 isotope

Learning Check Given a nuclear symbol, what does the top left number represent? What does the bottom left number represent?

Can we write isotopes in a different way? You can also use the mass number and the name of the element to designate the atom or isotope This is called hyphen notation For example, two isotopes of carbon are carbon-12 and carbon-13 The nuclear symbols for these two isotopes would be: C 12 6 13 6 C

Learning Check What does the number after the hyphen represent?

What do the numbers used when writing isotopes represent? The mass number 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.

How do I figure out the number of neutrons when writing isotopes? To determine the number of neutrons in a specific isotope subtract the atomic number from the mass number See the formula below Mass Number (neutrons + protons) Atomic Number (number of protons) (number of neutrons)

Learning Check Boron consists of two isotopes, B-10 and B-11 1.) Determine the number of neutrons in each of the isotopes 2.) Using the periodic table, write the nuclear symbol for each isotope given in hyphen notation a.) B-10: 10 – 5 = 5 neutrons b.) B-11: 11 – 5 = 6 neutrons

What does the atomic weight of an element depend on? To identify isotopes the mass number is placed after the element’s name Ex: chlorine-35 potassium-37 The atomic weight of an element depends on the abundance of its isotopes. If you know the mass of the isotopes and the percent (fractional) abundance of the isotopes, you can calculate the element's atomic weight.

How do I calculate the atomic mass of an element based on percent natural abundance and isotopic masses? Example: Chlorine has 2 naturally occurring isotopes To calculate the average atomic weight: add the mass of each isotope multiplied by its percent abundance This is the solution for chlorine: (34.968852) * (0.7577) + (36.965303) * (0.2423) = 35.45 amu Mass # Mass Percent Abundance 35 34.968852 75.77 37 36.965303 24.23

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