OUTLINE of TOPICS The Atom The Elements Counting Atoms Periodic Groups Electron Configuration

The Atom What does it mean for a submarine to “submerge” underwater? What is a subscript? What are “sub”-atomic particles?

OBJECTIVE: Proton, Neutron, Electron 1. The Atom OBJECTIVE: Proton, Neutron, Electron

Atom made up of smaller parts 1. The Atom Atom made up of smaller parts These parts are called SUBATOMIC particles

are small things that make up an atom 1. The Atom SUBATOMIC particles are small things that make up an atom

Three types of SUBATOMIC Particles 1. The Atom Three types of SUBATOMIC Particles Proton Neutron Electron

1. Proton Has a POSITIVE charge Located in the nucleus 1. The Atom SUBATOMIC PARTICLES 1. Proton Has a POSITIVE charge Located in the nucleus

Has a NEGATIVE charge Smallest of the three Least mass of the three 1. The Atom SUBATOMIC PARTICLES 3. Electron Has a NEGATIVE charge Smallest of the three Least mass of the three NOT in the nucleus

Has the largest mass of the three 1. The Atom SUBATOMIC PARTICLES 2. Neutron Has NO charge Has the largest mass of the three Located in the nucleus

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom

1. The Atom Which subatomic particles are found in the nucleus? Questions to answer the video Which subatomic particles are found in the nucleus? What is in between the nucleus of an atom and the electron(s)? Where is most of the mass of an atom found? Why is most of the mass of an atom found there?

1. The Atom Summary & Review What are subatomic particles? What are the names, locations and charges of the three of subatomic particles? What is between the nucleus and the electron(s)? Where is most of the mass in an atom located? Why?

What type of information is given about carbon? The Elements Find Carbon on your Periodic Table What type of information is given about carbon?

OBJECTIVE: Quantitative data about elements and atoms 2. The Elements OBJECTIVE: Quantitative data about elements and atoms

2. The Elements What makes a gold atom different from a silver atom? Answer: the number of subatomic particles Better answer: the number of protons

The most important subatomic particle for the IDENTITY 2. The Elements The most important subatomic particle for the IDENTITY of an atom is the number of PROTONS

2. The Elements ATOMIC NUMBER = # of protons Each type of atom has its own ATOMIC NUMBER This number NEVER changes

ATOMIC NUMBER = # of protons 2. The Elements ATOMIC NUMBER = # of protons Example: Atom with 2 protons is a helium atom Atom with 6 protons is a carbon atom

2. The Elements ATOMIC NUMBER = # of protons Atomic number also tells us # of electrons WHY? Because the + and – must balance

6. The Periodic Table MASS NUMBER = # of protons PLUS neutrons Mass number =/= Atomic Mass Mass Number - Atomic Number Number of Neutrons This is NOT Mass Number

2. The Elements How many protons is a copper atom? Practice using Atomic and Mass Numbers The symbol for Copper is Cu How many protons is a copper atom? Atomic Number = Number of protons Find Copper on Periodic Table So answer = 29 protons

2. The Elements 2. How many electrons in a copper atom? Practice using Atomic and Mass Numbers The symbol for Copper is Cu 2. How many electrons in a copper atom? Atomic Number = Number of protons Atomic Number = number of electrons So answer = 29 electrons

Copper’s atomic number is 29, and has 35 neutrons. 2. The Elements Copper’s atomic number is 29, and has 35 neutrons. 3. How many neutrons in this copper atom? Mass Number = # of Protons + # of Neutrons Mass Number = 29 + 35 64-29 = 35 Neutrons

2. The Elements Practice using Atomic and Mass Numbers Copper’s atomic number is 29, and the mass number is 64. How many protons in a copper atom? Atomic Number = Number of protons So answer = 29 How many electrons in a copper atom? Atomic Number = Number of protons Atoms are neutral, so number of protons = number of electrons How many neutrons in this copper atom? Mass Number – Atomic Number = Number of Neutrons Mass Number = 64, and Atomic Number = 29 64-29 = 35 Neutrons 11 protons, 11 electrons 27 80 131, 133

11 5 O 16 7 8 Pb 122 2. The Elements Atomic Symbol Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons 11 5 O 16 7 8 Pb 122

2. The Elements

Atoms of the SAME element can have different number of NEUTRONS. 2. The Elements Telling Atoms Apart Atoms of the SAME element can have different number of NEUTRONS.

2. The Elements Atoms of the SAME element can have different number of NEUTRONS These types of atoms are called ISOTOPES Iso = same Tope = place

2. The Elements How many protons? How many neutrons? What is the mass number?

2. The Elements How many protons? How many neutrons? What is the mass number?

2. The Elements Purpose of this slide is to show nomenclature and format for writing isotopes.

Different atoms can have the same MASS NUMBER. 2. The Elements Telling Atoms Apart Different atoms can have the same MASS NUMBER. 17 protons, 17 electrons, 18 neutrons, 20 neutrons 20 protons, 20 electrons, 22 neutrons, 24 neutrons EMPHASIZE: WHICH PARTICLE IS CHANGING?

2. The Elements They CANNOT have the same ATOMIC NUMBER EX: Different atoms can have the same MASS NUMBER They CANNOT have the same ATOMIC NUMBER EX: Copper Zinc Atomic Number = 29 Atomic Number = 30 Neutrons = 36 Neutrons = 35 Mass Number = 65 Mass Number = 65

Draw models of the of two isotopes: 2. The Elements Summary & Review Draw models of the of two isotopes: carbon-12 carbon-13 Your drawings should have the correct number of protons, neutrons, and electrons Atoms can have different number of NEUTRONS = Isotope They can also have different number of ELECTRONS = Ions IDENTITY is based on # of Protons. This does NOT change

How many donuts in one dozen? How many flowers in one dozen? Counting Atoms How many donuts in one dozen? How many flowers in one dozen? How many eggs in one dozen? Does it matter?

OBJECTIVE: Converting Units with Atoms 3. Counting Atoms OBJECTIVE: Converting Units with Atoms

3. Counting Atoms Dozen = unit of measurement MOLE is also a unit of measurement

1 mole : 6.02 x 1023 3. Counting Atoms Just like 1 dozen = 12 1 mole = 602 000 000 000 000 000 000 000 1 mole : 6.02 x 1023

1 mole = 6.02 x 1023 3. Counting Atoms 1 mole of donuts = 1 mole of flowers = 602 000 000 000 000 000 000 000 flowers

We use MOLE to count number of atoms 3. Counting Atoms 1 mole = 6.02 x 1023 We use MOLE to count number of atoms

1 mole = 6.02 x 1023 6.02 x 1023 copper atoms 3. Counting Atoms Example: 1 mole of Copper atoms = 602 000 000 000 000 000 000 000 copper atoms 6.02 x 1023 copper atoms

C.F. 1 mole : 6.02 x 1023 atoms 3. Counting Atoms 6.02 x 1023 = Avogadro’s Number C.F. 1 mole : 6.02 x 1023 atoms Convert 3.27 moles of Fe, iron, into number of atoms. Convert 7.23 moles of O, oxygen into number of atoms.

3. Counting Atoms How do we get moles? We get moles from MOLAR MASS Where do we get MOLAR MASS? We get Molar Mass from Atomic Mass Where do we get Atomic Mass? We get Atomic Mass from Periodic Table This is NOT Mass Number

Atomic Mass = Molar Mass = 1 Mole 3. Counting Atoms Atomic Mass = Molar Mass = 1 Mole in AMU in grams Example: Carbon: Atomic mass = 12.01 AMU so Molar Mass of Carbon = 12. 01 g so 12.01 g of Carbon = 1 mole of Carbon This is NOT Mass Number

2 Conversion Factors for mole 3. Counting Atoms 2 Conversion Factors for mole C.F. 6.02 x 1023 atoms : 1 MOLE C.F. 1 MOLE : molar mass

3. Counting Atoms Question gives you grams and asks for number of atoms Convert grams to Moles Convert moles to # of atoms C.F. Molar Mass = MOLE = 6.02 x 1023 atoms Question gives you number of atoms and asks for mass in grams Convert # of atoms to moles Convert moles to grams C.F. 6.02 x 1023 atoms = MOLE = Molar Mass

3. Counting Atoms Summary & Review What is the unit of measurement for counting atoms? What is Avogadro’s number? What is the conversion factor for mole and # of atoms? Where do we get molar mass? What is the unit for molar mass? What is the conversion factor for mole and mass?

OBJECTIVE: Learn 5 groups/families 4. The Periodic Table OBJECTIVE: Learn 5 groups/families

4. Periodic Groups Important GROUPS Alkali Metals Alkali Earth Metals Halogens Noble Gases Transition Metals Lanthanides Actinides Metalloids

metals VERY reactive in water 4. The Periodic Table GROUP 1 Alkali Metals metals VERY reactive in water

4. The Periodic Table Group 2. Alkali Earth Metals metal not as reactive

4. The Periodic Table Groups 3-12: Transition Metals conducts heat and electricity malleable – like Playdoh

4. The Periodic Table Group 17: Halogens non-metal very reactive

4. The Periodic Table Group 18: Noble Gases gases not reactive

4. The Periodic Table Metalloids solid, but not metal has properties of metals

4. The Periodic Table Lanthanides & Actinides extremely rare radioactive

5. Electron Configuration There are 4 types of orbits/orbitals S orbital P orbital

5. Electron Configuration There are 4 types of orbits/orbitals D orbital

5. Electron Configuration There are 4 types of orbits/orbitals F orbital

5. Electron Configuration There are 4 types of orbits/orbitals We are only going to use the s p d orbitals

5. Electron Configuration

5. Electron Configuration What is the difference between 1s orbital and 2s orbital?? size (draw) VIDEO

5. Electron Configuration What do the orbits/orbitals represent? What does it mean for orbits to be quantized? What are the three orbitals we will use? What is the different between a 1s orbital and a 2s orbital? What is the difference between a 2p and a 3p orbital? What do the number and the letter represent in “1s” and “2p”?

What did we learn? Why are the following people important: Democritus, Boyle, Lavoisier, Proust, Dalton? Explain the Law of Conservation of Mass Explain the Law of Definite Proportion, aka the Big Mac Law Explain the Law of Multiple Proportion, aka In-N-Out Cheeseburger vs Double-Double Law What are subatomic particles, and what are the charges & location of each?

What did we learn? Why is Thomson important? Be able to draw, label, and explain Thomson’s setup Be able to explain Thomson’s conclusion Be able to explain Thomson’s model of the atom. What two things about the electron did Millikan discover? Be able to draw, label, and explain Millikan’s setup What two forces did Millikan balance Be able to perform Millikan’s calculation Why is Rutherford important? Be able to draw, label, and explain Rutherford’s setup Be able to explain Rutherford’s conclusions How is Rutherford’s model of the atom different from Thomson’s?

What did we learn? What does the atomic number represent? What does the mass number represent? Be able to find the number of protons, neutrons and electrons using the atomic and mass numbers Be able to convert # of atoms into moles Be able to convert moles into grams Be able to convert grams to # of atoms Be able to convert # of atoms to grams