The structure of the atom

Slides:

Advertisements

Similar presentations

Reviewing Subatomic Particles

Advertisements

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

Subatomic Particles Atomic Number | Isotopes | Ions.

Atomic Structure Section The Nucleus Nucleus- contains most of the mass of an atom – Protons & Neutrons contains most of an atom’s mass – Electrons-

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!

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.

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.

Atomic Structure I. Subatomic Particles.

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

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.

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

Atoms and Molecules Atom is smallest particle that can be identified as a particular substance. Molecule is two or more atoms bonded to each other.

The three SUBATOMIC PARTICLES are

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

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)=

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.

The Basics of Atomic Structure. Terms you should know… Atom: smallest unit of an element that maintains the identity of that element. Chemical Reaction:

Proton, Neutron, Electron Counting Protons (p + ) are positively charged and located in the nucleus The number of protons in each atom can be found on.

Chapter 4.3 Distinguishing Among Atoms

Atomic Structure Unit 3.

ParticleSymbolRelative Charge Relative Mass (proton = 1) Actual Mass (g) Electrone-e- 1-1/ X Protonp+p x Neutronn0n x10.

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.

Atoms, Ions, & Isotopes pg & LO: I can explain the number of protons, electrons, neutrons & overall charge for any element or isotope.

Chapter 4 Atomic Structure. Atom Atom – smallest part of an element that retains the properties of that element. Atomic Theory – proposed by John Dalton.

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 Test Review 166 point total. 1.The atomic number is the number of protons. 2. The mass number is the number of protons and neutrons.

Atomic Number & Atomic Mass

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

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.

Rutherford’s Atom/Past Electrons orbit nucleus similar as planets to the sun Atom of the Present Electrons orbit nucleus in the form of clouds.

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

Atoms and Isotopes “Up and at them”. Atoms An atom is composed of a central nucleus which consists of protons and neutrons, along with orbiting electrons.

Atomic Structure What are atoms made of? How are atoms put together? What are Elements? Isotopes?

 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.

The Nuclear Atom Atoms differ from one another by their number of: 1.Protons 2.Neutrons 3.Electrons Electrons have a NEGATIVE charge. The MASS of an electron.

Notes on Isotopes Remember Protons are (+) and Electrons are (-). Neutrons were the last subatomic particles to be discovered because they have no electrical.

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

Protons, Neutrons, and Electrons

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

The Basics of Atomic Structure

 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.

Atomic Structure Review Which of the following is NOT true about electrons? a) They have a negative charge b) They are the heaviest subatomic particle.

UNIT 3: DAY 1 AND DAY 3 ATOMIC STRUCTURE. ATOM, ELEMENTS, AND COMPOUNDS Atoms are the smallest unit of matter In classification, all atoms are elements.

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

Subatomic Particles. Using the Periodic Table N Atomic Number Mass Number Symbol.

Link to Phet build an atom

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

1 The Atom Atomic Number and Mass Number Isotopes.

SECTION 4.3 HOW ATOMS DIFFER. PENNIES AS ATOMS MASS OF SAMPLE 1: MASS OF SAMPLE 2: IF THEY HAD THE SAME NUMBER OF PENNIES, WHY WERE THE MASSES DIFFERENT?

Atomic Structure Modern Atomic Theory.

Subatomic Particles Masses of Atoms Mass Number Isotopes Ions

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.

The Basics of Atomic Structure

Atomic Structure.

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

ATOMIC STRUCTURE Chapter 4.

Distinguishing Among Atoms

Isotopes and Ions.

Isotopes and Ions.

Presentation transcript:

The structure of the atom Chapter 4.3 How Atoms Differ

Atomic number The number of protons in an atom that identifies it as an atom of a particular element (also equals the number of electrons) Every element has a unique atomic number (unique number of protons that cannot be changed without change the identity of the element) Atomic number = number of protons = number of electrons In a neutral (no charge) atom, the number of electrons (- charge) always equals the number of protons (+ charge) The periodic table is organized left to right and top to bottom by increasing atomic number.

Atomic Number Problem Complete the following table: Element Atomic Number Protons Electrons 19 35 Ne 10 K 19 19 Br 35 35 10 10

Mass of atoms Measured in atomic mass units (amu) Based on carbon-12 as a standard 1 amu = 1/12 the mass of the carbon-12 atom Masses of subatomic particles: Electron = 0.000549 amu Proton = 1.007236 amu Neutron = 1.008665 amu

Mass number Mass number = number of protons + number of neutrons How heavy the atom is Nucleus is heaviest - Contains protons and neutrons Mass number = number of protons + number of neutrons A single element can have different mass numbers if there is more than one “version” of the element – called an isotope

Isotopes Atoms of the same element with the same number of protons but different numbers of neutrons. The mass of isotopes increases with increasing neutrons but chemical behavior stays the same Chemical behavior is determined only by the the number of electrons that an atom has.

Isotope identification Each isotope of an element is identified with the mass number Copper-63 (Cu-63): mass number = 63 (29 protons + 34 neutrons) Copper-65 (Cu-65): mass number = 65 (29 protons + 36 neutrons) Atomic Mass: the weighted average mass of all of the isotopes of a particular element This is the mass number listed on the periodic table with decimal places!!!

(Protons or electrons) Isotope notation*** Isotopes are often written using a notation involving the chemical symbol, atomic number, and mass number Mass Number (Protons + Neutrons) Copper-65 63 Cu 65 Cu 29 29 Copper-63 Atomic Number (Protons or electrons)

Isotope problem: Determine the number of protons, electrons and neutrons for the isotopes in the table below; name each isotope and write its symbol Element Atomic Number Mass Number a. Neon 10 22 b. Calcium 20 46 c. Oxygen 8 17 d. Iron 26 57 e. Zinc 30 64 f. Mercury 80 204

Calculating Atomic Mass Atomic mass: the weighted average mass of all of the isotopes of that element Mass of each isotope and isotope abundances are required to calculate this Isotope abundances Amount of element isotopes that readily exist (presented as percentages)

CALCULATING Atomic Mass An element has 3 isotopes with the following mass numbers and abundances: 23A: mass 23 amu; abundance 7% 25A: mass 25 amu; abundance 76% 26A: mass 26 amu; abundance 17% (23 x 0.07)+(25 x 0.76)+(26 x 0.17) = 25.03

Isotope Mass (amu) Percent Abundance Atomic Mass Problem: Calculate the atomic mass of the element X and identify the element from the periodic table knowing that it has the isotopes listed in the table below Isotope Mass (amu) Percent Abundance 54X 53.940 5.9% 56X 55.935 91.72% 57X 56.935 2.1% 58X 57.933 0.28%

Ion formation Ions are formed when atoms gain or lose electrons. Positive Ion formation When an atom LOSES one or more electrons When an electron (negative charge) is lost, the ion ends up with a net positive charge (Ca – 2 e- = Ca2+) Negative Ion Formation When an atom GAINS one or more electrons When an electron (negative charge) is gained, the ion ends up with a net negative charge (O + 2 e- = O2-)