The Modern Model The modern atom is composed of two regions: 1. Electron cloud- Most of the volume of an atom and is the region where the electron can.

Slides:

Advertisements

Similar presentations

Atoms and their structure

Advertisements

Atomic Structure and Bonding

Atomic Structure. What is an atom? Atom: the smallest unit of matter that retains the identity of the substance.

Atomic Structure Nucleus – contains protons and neutrons

OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM

Atomic Structure Standard Atomic Notation Isotopes Isotopic Abundance.

Calculating Atomic Mass

Subatomic Particles and Isotopes. Subatomic Particles Protons- Positively Charged Protons- Positively Charged Located in the nucleus Located in the nucleus.

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

Atomic Theory Modern Model. atom (page 313) smallest part of an element that has all the properties of the element.

Introduction to Chemistry for Allied Health Sciences Structure of the Atom Kirk Hunter Chemical Technology Department Texas State Technical College Waco.

Subatomic Particles, Atomic Number and Atomic Mass

Counting Atoms.

Atomic Structure I. Subatomic Particles.

Chapter 4 Atoms and their structure History of the atom n Not the history of atom, but the idea of the atom. n Original idea Ancient Greece (400 B.C.)

How do atoms differ? Section 4.3.

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

Virtually everything that is, is made up of atoms. Chapter 12, page 361 Balloon and sweeter animation.

Subatomic Particles.  subatomic-lower (or smaller) than an atom  Protons-positive particles  Neutrons-neutral particles  Electrons-negative particles.

How Atoms Differ.

Slide 1 Particles in the Atom. Slide 2 Electrons (-) charge no mass located outside the nucleus Protons (+) charge 1 amulocated inside the nucleus Neutron.

Chapter 4 Atoms and Their Structure History of the atom n Not the history of atom, but the idea of the atom n Original idea Ancient Greece (400 B.C..)

Atomic Structure Two regions of every atom: Nucleus -is made of protons and neutrons -is small and dense Electron cloud -is a region where you might.

1.3 Understanding Atomic Mass. A Review: Subatomic particles Electron Proton Neutron NameSymbolCharge Relative mass Actual mass (g) e-e- p+p+ nono +1.

Chapter 4 Atoms and their structure History of the atom n Not the history of atom, but the idea of the atom n Original idea Ancient Greece (400 B.C..)

Unit 2 Review - Section 1 Atomic Structure and Mass.

Counting Atoms 3.3. Counting Atoms Very difficult to count Atomic Number – # of p + of each atom of that element Whole numbers Elements arranged by atomic.

Atomic Theory Chapter 2 Pg: State the position of protons, electrons and neutrons in the atom State the relative masses and relative.

Subatomic Particles. Atomic Particles ParticleChargeMass (kg)Location Electron9.109 x Electron cloud Proton x Nucleus Neutron

Isotopes Atoms of the same element with different mass numbers. Mass # Atomic # Nuclear symbol: Hyphen notation: carbon-12 Courtesy Christy Johannesson.

Chapter 4 “Atomic Structure”. “Animal Style” Atom.

Boxes on the Periodic Table What do they tell us??

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

Atoms Atom- the smallest part of an element Atoms of one element are different from another element. contains protons, electrons, and neutrons Atomic Mass.

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

Proton A positively charged subatomic particle (found in the nucleus). A subatomic particle with no charge (found inside the nucleus). Neutron.

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.

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.

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

Protons, Neutrons, and Electrons

Atomic Structure Chapter 4. Sizing up the Atom O Radii of most atoms: 5 x m to 2 x m O Copper penny contains 2.4 x atoms. The population.

Distinguishing Atoms Chapter 4 Section 3. Atomic Number Atoms are composed of identical protons, neutrons, and electrons –How then are atoms of one element.

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

Structure of the Atom There are two regions The nucleus With protons and neutrons –Positive charge –Almost all the mass Electron cloud –Most of the volume.

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.

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.

Atomic Structure Subatomic particles Electron Proton Neutron NameSymbolCharge Relative mass e-e- p+p+ nono +1 0 ~0 1 1 Electrons and protons have equal.

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.

Introduction to Atomic Theory. History of the atom Democritus (400 BC) suggested that the material world was made up of tiny, indivisible particles atomos,

Atoms and their structure

Dalton’s Atomic Theory (experiment based!)

Atomic Structure Modern Atomic Theory.

Subatomic Particles.

Atomic Structure.

Atomic Structure.

Atoms and their structure

Subatomic Particles.

Subatomic Particles.

4*3 TEST REVIEW.

ATOMS AND ATOMIC STRUCTURE Atom Nucleus Proton Neutron Electron

Warm Up 1.What did Rutherford’s scattering experiment show? Need to list 2 important findings. 2. What did Thomson discover? Describe the atomic model.

Atoms and their structure

0:56 0:55 0:54 0:53 0:57 0:58 1:02 1:01 1:00 0:59 0:52 0:51 0:44 0:43 0:42 0:41 0:45 0:46 0:50 0:49 0:48 0:47 1:03 1:04 1:19 1:18 1:17 1:16 1:20 1:21 1:25.

Atomic Structure Nucleons Atomic Number

ARE ALL ATOMS OF THE SAME ELEMENT IDENTICAL?

Atomic Number and Mass Number

Atomic Particles Particle Charge Mass (kg) Location Electron -1

Presentation transcript:

The Modern Model The modern atom is composed of two regions: 1. Electron cloud- Most of the volume of an atom and is the region where the electron can be found (extranuclear) 2. The nucleus – with protons and neutrons so that it has a Positive charge and almost all the mass

Major Subatomic Particles Atoms are measured in picometers, meters Hydrogen atom, 32 pm radius Nucleus is tiny compared to atom If the atom were a stadium, the nucleus would be a marble Radius of the nucleus is on the order of m Density within the atom is near g/cm 3 NameSymbolChargeRelative Mass (amu) Actual Mass (g) Electrone-e- 1/ x Protonp+p x Neutronnono x10 -24

Nuclear Symbols Every element is given a corresponding symbol which is composed of 1 or 2 letters (first letter upper case, second lower), as well as the mass number and atomic number E A Z elemental symbol mass number atomic number

Locations on periodic table… Atomic Number = number of protons (p + ) in the nucleus Determines the type of atom Li atoms always have 3 protons in the nucleus, Hg always 80 Mass Number = number of protons + neutrons Electrons have a negligible contribution to overall mass In a neutral atom there is the same number of electrons (e - ) and protons (atomic number)

Find the Find the number of protons number of protons number of neutrons number of neutrons number of electrons number of electrons atomic number atomic number mass number mass number W F 19 9 Br 80 35

If an element has an atomic number of 34 and a mass number of 78 what is the: If an element has an atomic number of 34 and a mass number of 78 what is the: number of protons in the atom? number of protons in the atom? number of neutrons in the atom? number of neutrons in the atom? number of electrons in the atom? number of electrons in the atom? complete symbol of the atom? complete symbol of the atom? If an element has 91 protons and 140 neutrons what is the: If an element has 91 protons and 140 neutrons what is the: atomic number? atomic number? mass number? mass number? number of electrons? number of electrons? complete symbol? complete symbol?

Isotopes Atoms of the same element can have different numbers of neutrons and therefore have different mass numbers The atoms of the same element that differ in the number of neutrons are called isotopes of that element H 1 1 Protium H 2 1 Deuterium H 3 1 Tritium

Naming Isotopes When naming, write the mass number after the name of the element Examples: carbon- 12 carbon -14 uranium-235

Average Atomic Mass Did you ever notice that the mass number on the periodic table is not a whole number? There are the decimal numbers on the periodic table. **This is because it is an average mass for all the isotopes of each atom

How heavy is an atom of oxygen? There are different kinds of oxygen atoms (different isotopes) 16 O, 17 O, 18 O We are more concerned with average atomic masses, rather than exact ones Based on abundance of each isotope found in nature We can’t use grams as the unit of measure because the numbers would be too small Instead we use Atomic Mass Units (amu) Standard amu is 1/12 the mass of a carbon-12 atom Each isotope has its own atomic mass

Calculating Averages You have five rocks, four with a mass of 50 g, and one with a mass of 60 g. What is the average mass of the rocks? Total mass = 4 x 50 g + 1 x 60 g = 260 g Average mass = (4 x 50 g + 1 x 60 g)/5 = (260 g)/5 = 52 g

80% of the rocks were 50 grams 20% of the rocks were 60 grams What is the average mass of the rocks? Average mass = 0.8 x x 60 = = 52 g Average = (% as decimal) x (mass 1 ) + (% as decimal) x (mass 2 ) + (% as decimal) x (mass 3 ) + … Calculating Averages when given %:

1.Calculate the av atomic mass of copper if copper has two isotopes 69.1% has a mass of amu The rest (30.9%) has a mass of amu 2.Magnesium has three isotopes 78.99% magnesium 24 with a mass of amu 10.00% magnesium 25 with a mass of amu The rest magnesium 26 with a mass of amu What is the atomic mass of magnesium? EXAMPLES:

If not told otherwise, the mass of the isotope is the mass number in amu The average atomic masses are not whole numbers because they are an average mass value Remember, the atomic masses the decimal numbers on the periodic table Average Atomic Masses

To do : Page 45 –Questions 1, 2, 3, 4 Page 46 –Questions 2, 3, 4, 5a