Atomic Theory Review Game

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

4.3: HOW ATOMS DIFFER ATOMIC NUMBER

Solving atomic calculations: Working with: – Elements – Isotopes – Ions – Atomic # – Atomic mass – Charge.

Unit 3: Atomic Structure Atomic Number, Mass Number, and Isotopes.

Atomic Mass & Number Isotopes The Periodic Table.

Atomic Structure I. Subatomic Particles.

Distinguishing Among Atoms

Revision Quiz Atomic Theory 1

HOW MANY PROTONS, ELECTRONS, AND NEUTRONS ARE IN AN ATOM?

Building Blocks 1c Int

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.

The Structure of the Atom. Modern Concept of Atomic Theory 1.Atom consists of a tiny nucleus 2.Electrons move in an area directly surrounding the nucleus.

Determining the NUMBER of Protons Electrons and Neutrons in Atoms, Ions, and Isotopes.

Isotopes and Ions. Fill in the following table: Symbol Atomic Mass Atomic Number # of protons # of neutrons # of electrons Na Na Ne Ne Hg Hg Zn Zn Al.

Atom Review 1.What are the 3 subatomic particles? 2.What atom is the amu based on? 3. What is located in the nucleus of the atom? 4. What is the nuclear.

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

Isotopic Abundance SCH 3U. Atomic Mass The mass of an atom (protons, neutrons, electrons) Relative Atomic Mass: An element’s atomic mass relative to the.

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.

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.

D. Subatomic Particle & the Nuclear Atom 1.Nucleus contains positively charged protons and neutral neutrons VERY dense! If a nucleus were the size of the.

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.

Atomic Mass. Each element found on the periodic table of elements is given an atomic mass The atomic mass tells you the average mass of the atoms of an.

Atoms. Structure of Atoms  Atoms are made up of subatomic particles:

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”. 

ELECTRONS. Review Electrons were discovered by ______________ Electrons have a ___________ charge Electrons are located…. Outside of the nucleus in an.

Chapter 8 Earth Chemistry Part – Atomic Number  An atom of a specific element is different from other elements by the number of protons it has.

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

Isotopes Chapter 4, Section 3 Pg Review of Atoms Atoms are made of protons, neutrons, and electrons. – Protons are +, electrons are –, and.

1 The Atom Atomic Number and Mass Number Isotopes.

Do Now: Match the scientist with their contribution to the atom A. Dalton1. Mass of electron B. Thomson2. atomic theory C. Milikan3. discovered electron.

Chapter 4 Atomic Structure 4.1 Defining the Atom

Masses of Atoms.

Chapter 3: Chemical Foundations: Elements, Atoms, and Ions

Section 2 Protons, neutrons, and electrons- how atoms differ

Calculating Atomic Mass

Calculating Average Mass

Atomic Particles Particle Charge Mass # Location Electron -1

Standard Atomic Weights on Periodic Table (red numbers) are found through the terrestrial (Sol III) relative abundances of the masses (in amu) of the isotopes.

Presentation Properties of Atoms

Ch. 4/5 Notes Day 3 1/28/16.

Section 1 Structure of the atom and cells on the periodic table

Warmup Draw an atom.

Chapter 4 Atomic Structure 4.1 Defining the Atom

Structure of an Atom.

Elements, Isotopes and More

How Atoms Differ Chp 4.

Chapter 4 Atomic Structure 4.1 Defining the Atom

What is an isotope? Review Video.

Chapter 4 Atomic Structure 4.1 Defining the Atom

Distinguishing Among Atoms

Standard Atomic Weights on Periodic Table (red numbers) are found through the terrestrial (Sol III) relative abundances of the masses (in amu) of the isotopes.

Atomic Symbols = = mass # atomic # protons + neutrons protons

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

Atomic Structure Nucleons Atomic Number

Isotopes & Ions.

Atomic Math Calculations

Atomic Structure Review Foldable

How We Know What We Can’t See Looks Like Day 4 Average Atomic Mass

Atomic Structure Nucleus Protons Neutrons Electrons.

Presentation transcript:

Atomic Theory Review Game

Complete the sentence: Isotopes are forms of an element that have ____________________________

What are the key features of the Bohr model of the atom?

Draw an atom that has the following features: mass number 27 5 more electrons than oxygen

Calculate the weighted average atomic mass of neon from the following data: Isotope % abundance mass Ne-20 90.48% 19.9924356 Ne-21 0.27% 20.9938428 Ne-22 9.25% 21.9913831

How many electrons are in a sodium ion with a +1 charge? Atoms Protons Neutrons Electrons Mass Number Sodium 12 23

Describe the composition of an atom of this isotope.

How does the composition of an atom of Cu differ from the composition of a Cu2+ ion?

Where does most of the mass come from in an atom Where does most of the mass come from in an atom? Where does most of the volume come from in an atom?

Define an atom.

How is a nuclear reaction different from a chemical reaction?

Which element is this and what is its mass number?

Which are the protons and which are the neutrons?

Complete the following table for a neutral atom: Element Protons Neutrons Electrons Mass # 24 52 22 41

What is the charge of each? atom electron proton neutron

What aspects of Dalton’s atomic theory were incorrect?