Intro to Chapter 4 We are finally learning about the atom! Please have out last night’s homework. On the back of your homework divide your paper into two.

Slides:



Advertisements
Similar presentations
4.3: HOW ATOMS DIFFER ATOMIC NUMBER
Advertisements

Average Atomic Mass. How much does an atom weigh?  Protons & Neutrons:  1.67 X gram  Electrons:  9.10 X gram  To avoid working with.
Chapter 11B Notes Determining Isotope Masses. Intro What is the mass of an atom with 6 protons and 6 neutrons? 12 What is the mass of an atom with 6 protons.
ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons A Z X A = mass number (the total number of protons.
OF PROTONS, NEUTRONS AND ELECTRONS IN AN ATOM
Isotopes & Average Atomic Mass
Atoms: The building blocks of Matter
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.
 Atoms of the same element are NOT exactly similar  They may have different masses ◦ Vast majority of mass is from protons and neutrons  Element is.
Subatomic Particles  Protons and electrons are the only particles that have a charge.  Protons and neutrons have essentially the same mass.  The mass.
Section 3 Counting Atoms Lesson Starter Imagine that your semester grade depends 60% on exam scores and 40% on laboratory explorations. Your exam scores.
Distinguishing Among Atoms
Isotopes Atoms of the same element that different mass numbers
1. I have 22 neutrons and a mass of I have 37 protons and 39 electrons. 3. I have 22 neutrons and 19 protons.
Candium Lab.
+ Atomic Structure and Periodic Table Sierra Larsen Karsen DeJarnett Briauna Jones.
Unit 3: Atomic Theory & Structure Section 2 – Distinguishing Among Atoms.
THE ATOM Counting. The Atom- September 5  Pick up a Chemistry textbook from the shelf  Take out one piece of notebook paper, write your name, date,
Number of Protons = Number of Electrons Number of Protons = Atomic Number Atomic Mass = Protons + Neutrons.
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.
Law of Conservation of Mass Law of Definite Proportions.
More about isotopes Atomic mass vs average atomic mass or atomic weight.
& Average Atomic Mass  Atoms with the same number of protons (they are the same element) but different number of neutrons.
Unit 3: Atomic Structure Atomic Mass Units (amu) and Calculating Atomic Mass.
 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.
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.
Friday October 1, 2015 TO DO RIGHT NOW: 1.Get out your HW and PT 2.Copy words on page 42 3.Update your table of contents HOMEWORK Due Monday- Isotope Worksheet.
Chapter 4 Section 4.  There are about 118 known types of atoms.  Each element has it’s own type of atom.  All atoms of an element have to have one.
Section 4.3 How Atoms Differ. Objectives Explain the role of atomic number in determining the identity of an atom Define an isotope and explain why 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.
…AND THE AVERAGE ATOMIC MASS Isotopes. PG 88 GENERAL- ATOMS OF THE SAME ELEMENT BUT HAVE DIFFERENT AMOUNTS OF NEUTRONS IN THE NUCLEUS PAGE 54 PRE AP ATOMS.
Chapter 3 Average Atomic Mass. Section 3 Counting Atoms Relative Atomic Masses The standard used by scientists to compare units of atomic mass is the.
Atomic Mass and Isotopes. Review Quiz ParticleChargeMassLocationSymbol Electron Proton Neutron.
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.
Calculating Particles in a atom
Atomic Masses Test Friday!. Atomic Mass is an average (decimal) An average of known isotopes for an element The atomic mass of an element is closest to.
Chapter 3 Preview Lesson Starter Objectives Atomic Number Isotopes
Atomic Structure. I. Atoms The atom is the basic unit of matter.
Calculating Particles for an ion. Representations from the Periodic Table Fe Iron Oxidation States Name Atomic Mass Atomic Number.
1Chemistry Chapter 4: How Atoms Differ: Atomic number = # p + AND e - (assume neutral atom for charge). Atomic number = # p + AND e - (assume neutral atom.
Atomic Structure. Subatomic Particles In the nucleus: Protons Mass  1 amu Charge = +1 Neutrons Mass  1 amu Charge = 0 In the electron cloud: Electrons.
Isotopic Abundance Pages Thinking question Why are there decimal places for atomic masses on the periodic table if protons and neutrons have amu.
Ch. 3-3a Distinguishing and Counting Atoms. POINT > Define Atomic Number POINT > Define Mass Number POINT > Describe and identify isotopes POINT > Determine.
Isotopes and abundance. The relative atomic mass scale is now based on an isotope of carbon, carbon-12, which is given the value of amu.
Daily Science Who discovered the electron and how did he discover it? What was his model called? What tells you the number of p + an element has? Write.
Isotopes are atoms of the same element that have a different number of neutrons For example, Hydrogen has 3 isotopes: Protium (0 neutrons) Deuterium (1.
Atomic Structure atomic number atomic mass elemental symbol.
Chemistry – Oct 24, 2016 P3 Challenge- Objective –
Ch. 3-3a Distinguishing and Counting Atoms
Calculating Average Mass
Day 5 Chapter 4 Section 2 and 3.
Atomic Structure.
A B 21085At Fe Mo 5827Co 3216S Pb4+ Symbol
Day 5 Chapter 4 Section 2 and 3.
Unit 2: Atomic Theory & Structure
Atomic Structure Walk Around
Distinguishing Between Atoms
How do structures of atoms Differ?
Atomic number, atomic symbol, mass number, isotopes
Atomic Structure.
Mass of Individual Atoms
Do First Actions: Get the 4 sheets: Atomic Structure Interactive, Calculating Protons, Neutrons, and Electrons Sheet, Bohr Model worksheet and It’s Natural.
Elements, Isotopes and More
How Atoms Differ Chp 4.
Subatomic particles What information would you get about an element from the periodic table?
Calculating Average Atomic Mass
Atomic Math Calculations
Chemistry Chapter 3 Section 3
Presentation transcript:

Intro to Chapter 4 We are finally learning about the atom! Please have out last night’s homework. On the back of your homework divide your paper into two sections. Title the first section “K” and the second “L”. -In the first section labeled “K”, write down everything you think you know about atoms and the periodic table. Homework: Read 4.2 do # 8-10, 12,13

Entrance Ticket 9/22/14 Please have out your 4.1 and 4.2 homework 1.) Draw what you think an atom looks like and label it 2.) What was Rutherford’s conclusion from the gold foil experiment?

Entrance Ticket 9/23/14 This is the symbol for the isotope of gold that has a mass number of 197 and gold’s atomic number is ) How many protons does a gold atom have? 2.) How many electrons does a gold atom have? 3.) How many neutrons does this isotope of gold have?

-Write the symbol for the isotope of carbon that has 8 neutrons. (use the periodic table for atomic #)

Entrance Ticket 9/24/14 1.) How many protons, neutrons and electrons are in an atom of Copper that has a mass number of 65? 2.) Write the symbol for the isotope of Krypton that has 58 neutrons. Please tear out your isotopes lab (p.12).

Answers 1.) Copper-65 has 29 protons, 29 electrons and 36 neutrons. 2.)

Isotopes Lab -If these were a real isotopes, all the brown beans would weight the same, but they don’t. This is the same for the white beans and popcorn kernals. -We will find how much each isotope weighs on average and pretend that they all weigh that much.

-Grades were updated and posted yesterday you can go look at them. -Please get out your isotopes lab.

Lead’s Average Atomic Mass Pb x = 2.9 Pb x = 49.6 Pb x = 45.7 Pb x =

Entrance Ticket 9/26/14 1.) What is average atomic mass? 2.) Where is it found? 3.) How is average atomic mass different than the mass number of an isotope? 4.) How is average atomic mass calculated?

Answers 1.) Average atomic mass is the weighted average of all the isotopes of an element. 2.) Ave. atomic mass is found on the periodic table. 3.) Mass # is the exact number of protons plus neutrons of an isotope. The ave. atomic mass is an average of the mass #s of all the isotopes of an element. 4.) Ave. atomic mass is calculated by taking the mass of each isotope times its abundance, and then adding those values. 4.) Ave. atomic mass is calculated by taking the mass of each isotope times its abundance, and then adding those values.

Entrance Ticket 9/29/14 Pass up entrance ticket #2! 1.) Please describe how you can find the number of protons, neutrons and electrons for a given isotope. 2.) Please write the isotope symbol for sodium- 23. How many protons, neutrons and electrons does it have? Homework: Read 5.1

Answers 1)The atomic # tells us the number of protons and electrons. Subtract the atomic # from the mass # to find the amount of neutrons. 2)Sodium-23

Entrance Ticket 9/30/14 Please get out last week’s 4.1 & 4.2 homework Please get out last week’s 4.1 & 4.2 homework 1.) Please write the symbol for the isotope Potassium ) If electrons are so small that we do not count their mass, why are they important?

Entrance Ticket 10/1/14 Please have out yesterday’s handout 1.) What are valence electrons? 2.) Why are valence electrons so important? Honors: Read and outline 5.2

Entrance Ticket 10/2/14 (1) Which atom has the electron configuration of: configuration of: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 (2) Please write the electron configuration for Iron (Fe). configuration for Iron (Fe).

Entrance Ticket 10/3/14 1. Which atom has the electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 ? a.) What is the short hand notation for writing this electron configuration? b.) How many valence electrons does this atom have? 2. What is the short cut to find the valence electrons for “s” & “p” block elements?

Fireworks Lab -Do not take the beaker with you! -Use a little bit of water and dab the tip of the Q-tip into the salt. Try to use both sides of Q-tip. -Put the tip into the Bunsen burner flame. DO NOT touch the Q-tip to the Bunsen Burner!

Entrance Ticket 10/6/14 DO NOT WRITE THIS E.T.! -Please have out your Fireworks Lab -What did the lab have to do with electron configurations? -Why do different metals emit (release) different colors when the are burned?

Study Guide Answers Matching 1.J M.C.19. B 2.G11. C20. B 3.A12. D21. C 4.C13. C22. D 5.F14. C23. C 6.E15. D 7.D16. A 8.B17. B 9.H18. A 10. I

Study Guide Answers #24.) Take the % abundance of each isotope and change it to a decimal. Multiply the abundance times the mass for each isotope and then add all those values. You should get amu

Study Guide Answers 25) a) 1s 2 2s 2 2p 6 3s 2 b) 1s 2 2s 2 2p 6 3s 2 3p 3 b) 1s 2 2s 2 2p 6 3s 2 3p 3 c) [Ar] 4s 2 3d 10 4p 5 c) [Ar] 4s 2 3d 10 4p 5 d) [Kr] 5s 2 4d 10 5p 6 d) [Kr] 5s 2 4d 10 5p 6 26) a.) Sulfur 26) a.) Sulfur b.) Neon c.) Scandium

Due right now! 1.) Fireworks labs!

Due right now! 1.) Fireworks labs! 2.) Electromagnetic wave problems. If your work is on more than one page, please turn it in stapled.