Anatomy of the Atom Atomic Structure.

Slides:

Advertisements

Similar presentations

Isotope Notation Isotope Notation uses a symbol to convey information about an isotope of a particular element. 23 Na 11.

Advertisements

Atomic Structure. Modern Atomic Theory Atom – smallest particle of an element that retains the properties of the element Subatomic Particles –Protons.

1.1 The Nature of Atoms Learning Goals determine the number of protons, electrons and neutrons in an atom or ion... distinguish between a cation.

OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM

Objectives:  1. Name and describe the three subatomic particles in an atom.  2. Determine the number of protons, neutrons, and electrons in an atom or.

Atoms, Ions and Isotopes. 2 Subatomic Particles ParticleSymbol Charge Relative Mass Electron e Proton p Neutron n0 1.

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

Atoms, Ions and Isotopes. 2 Subatomic Particles ParticleSymbol Charge Relative Mass (amu) Electron e Proton p Neutron n0 1.

Ions An atom that carries an electrical charge is called an ion If the atom loses electrons, the atom becomes positively charged (because the number of.

Atomic Structure. Modern Atomic Theory Atom – smallest particle of an element that retains the properties of the element Subatomic Particles –Electrons.

Isotopes and Ions.

Isotopes and Ions.

 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 3 Section 3 Counting Atoms Isotopes and Ions.

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

Atomic Structure. I. Atoms The atom is the basic unit of matter.

Isotopes and Ions. Isotopes Atoms of the same element that have different masses Have the same number of protons and electrons but different numbers of.

1Chemistry Chapter 4: How Atoms Differ: Atomic number = # p + AND e - (assume neutral atom for charge). Atomic number = # p + AND e - (assume neutral atom.

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

Structure of an Atom Atoms are composed of 3 subatomic particles: 1.Protons (p + ) – Positively charged, found in the nucleus, number of protons determines.

ATOMS, IONS, AND ISOTOPES QUICK REVIEW Atoms are made up of three particles:  Protons  Neutrons  Electrons Question: Which of the three particles.

Atomic Structure and Isotopes. Recap: Atomic Structure An atom is the simplest form of an element that can take part in a chemical reaction Three subatomic.

Atoms, Ions and Isotopes

Basic Atomic Structure

Atoms, Ions and Isotopes

Introduction to Atoms – Chapter 11

Atoms, Ions and Isotopes

Atomic Structure Modern Atomic Theory.

Counting Atoms.

II. Masses of Atoms Mass Number

Calculating Average Mass

Isotopes vs. Ions.

Neutrons Protons Electrons.

Atomic Structure Subatomic Particles C. Johannesson.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

Unit 3 – Atoms, Ions, Isotopes

Atomic Structure.

Isotopes and Ions Do Now – Explain how atoms of different elements differ from one another. Give a specific example.

Isotopes and Ions Section 3-3 Continued.

Isotopes and Average Atomic Mass

I have 8 protons, 8 neutrons, and 10 electrons.

Chapter 3 Objectives Explain what isotopes are.

Atomic Structure d. Atomic Structure d Atomic Structure d Electron (negative) Neutron (neutral) Proton (positive) d nucleus.

Atomic Structure.

Atomic Variation.

Calculating PEN (protons, electrons, neutrons) for Atoms and Ions

Structure of The Atom Not the Adam.

Foldables: Atoms Terms.

Warm Up What are the particles that make up the atom?

Warmup Draw an atom.

Introduction to Atoms – Chapter 11

Atomic Structure.

Elements, Isotopes and More

Protons, Neutrons, Electrons/Isotopes/Average Atomic Mass

Unit 3 “Atomic Structure”

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

Unit 3 “Atomic Structure”

Atoms, Isotopes and Ions

Atoms and their structure

ATOM COMPOSITION The atom is mostly empty space

Chapter 2 Matter is made up of Atoms

Basic Atomic Structure

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

Isotopes and Ions.

Ions and Ionic Bonds.

Isotopes and Ions.

Isotopes and Ions of Atoms

Presentation transcript:

Anatomy of the Atom Atomic Structure

Forces in the Nucleus The nucleus is positive (p+ and no) REMEMBER: The nucleus is positive (p+ and no) Like charges repel each other…so shouldn’t the p+ in the nucleus repel each other? But…when 2 p+ are close together in the nucleus there is a strong attraction between them. The same holds true for neutrons.

Atomic Number atomic number - the number of protons in the nucleus of each atom of a given element. The number of p+ identifies the element. Atomic Number increases from left to right on the periodic table.

Electrons The number of electrons in a neutral atom is equal to the number of protons in that atom. e- = p+

# of neutrons = mass number – atomic number mass number - the number of p+ & no in the nucleus of an atom. # of neutrons = mass number – atomic number

Isotope Notation Carbon-12 Nuclear Notation Hyphen Notation Uses the elements symbol followed by a hyphen & the mass number. C-12 Carbon-12

Example: Determine the number of p+, n0, and e- in an atom of Carbon-12.

Changes in the Atom Changing electrons

Electrons The number of electrons in a neutral atom is equal to the number of protons in that atom. e- = p+ Electrons can be lost or gained. This process is called ionization. When electrons are lost or gained, ions are formed.

Ions ion- an atom with a positive or negative charge. cation- an atom with a positive charge Cations are formed when an atom loses negatively charged electrons. Ca+2 is formed when calcium loses 2 electrons. Ca+2 has 2 less electrons than protons. the lithium atom the lithium ion

Ions anion- an atom with a negative charge Anions are formed when an atom gains negatively charged electrons. N-3 is formed when nitrogen gains 3 electrons. N-3 has 3 more electrons than protons.

Metals vs. Nonmetals Metals form cations. Na Na+ + 1e- Nonmetals form anions. Cl + 1 e- Cl-

Changes in the Atom Changing neutrons

Isotopes isotope- two or more atoms having the same atomic number (same #p+) , but different mass numbers (due to different #no). nuclide- general term for a specific isotope of an element.

Isotopes

How many protons, neutrons & electrons are there in the following? Cl-38 35Cl-1 Br-80 32S-2 N-14 56Fe+3

Atomic Mass Determination Average Atomic Mass - the weighted average of atomic masses of the naturally occurring isotopes of an element. The atomic mass is expressed relative to the value of exactly 12u for a carbon-12 atom. Atomic Mass Unit – amu or u

What is a weighted average? Example: Your grade in math might be 75% tests and 25% homework. What would your grade be if you had a test average of 80% and a homework average of 100%? Normally, you would average 80% & 100% to get 90%. However, with a weighted average, it is 85%.

Calculating Average Atomic Mass atomic mass of each isotope X percent natural abundance (in decimal form)

Percent Natural Abundance Percent Natural Abundance- the relative proportions expressed as percentages, in which isotopes of an element are found in nature.

Calculating Average Atomic Mass Ex: Uranium has two isotopes, uranium-235 and uranium-238. Uranium-235 has an atomic mass of 235.043amu and a percent natural abundance of 0.720%. Uranium-238 has an atomic mass of 238.050amu and a percent natural abundance of 99.280%. Calculate the average atomic mass of naturally occurring uranium.