CHAPTER 4: THE ATOM PHYSICAL SCIENCE
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1 CHAPTER 4: THE ATOM PHYSICAL SCIENCE By C. Goodman, Doral Academy Preparatory High School, Based on a PowerPoint presentation by Mrs. S. Temple, Doral Academy Preparatory High School
2 Essential Question Section 4.1 The Atomic Model What is the atomic model according to Rutherford, and how was it developed? (Explain the contributions of Democritus, Dalton, Rutherford and Thomson.)
3 Section 4.1 Vocabulary Democritus Atom Dalton Thomson Electron Rutherford Nucleus
4 Democritus atomic idea Democritus coined the term atom atomos = Greek word indivisible All substances are formed of atoms. Atoms are the smallest particles of matter
5 John Dalton ( ) English born Introduced his Atomic Theory in 1808 Based theories on Democritus work Dalton used experimental evidence.
6 Dalton s Atomic Theory What did Dalton add to the atomic theory? According to Dalton, all atoms of a given element were exactly alike, and atoms of different elements could join to form compounds.
7 Thomson the electron Thomson: discovered the electron Cathode ray tube experiment He concluded that all atoms have sub-atomic particles called electrons. The electrons are much smaller than the other parts of the atom They are negatively charged.
8 Rutherford the Nucleus Gold foil experiment Rutherford proposed that most of the mass of the atom was concentrated at the atom s center
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10 He was right. Rutherford conducted the gold-foil experiment. Rutherford discovered the nucleus. nucleus: an atom s central region, which is made up of protons and neutrons
11 Flowchart: atomic theory Democritus Atoms Can t be divided Dalton: Compounds Combinations of elements Thomson: Electron Also inferred proton Rutherford : Nucleus Inferred that the electrons orbit the nucleus
12 Essential Question Section 4.2 The structure of atoms 1. Compare and contrast the parts of the atom. 2. How are atoms and isotopes related? 3. What is a mole, and how is it related to average atomic mass? 4. Given an amount of a substance, how can one convert between the number of grams in the substance and number of moles, and vice versa?
13 Section 4.2 Vocabulary Proton Neutron Atomic number Mass number Isotope Unified atomic mass unit (AMU) Mole Molar mass
14 How small is small?
15 The Building Blocks of Matter Prions Quarks (6 Flavors) Protons Neutrons Electrons Atoms/ Elements Compounds
16 Atomic Number (Z) # of protons of each atom of that element Placed in increasing order on the Periodic Table This # IDENTIFIES the element How? Look on the periodic table!
17 Particles Symb ol Protons p + Positive charge Neutrons n 0 Neutral (no) charge Electrons e - Negative charge Charge Location Mass (amu) Nucleus 1 Nucleus 1 In area surrounding nucleus --
18 Nucleus and Electron Cloud Nucleus Positive charge because protons are positive and neutrons have no charge (neutral) Makes up most of atom s mass Electron cloud Region of space around nucleus; negative charge because of electrons Make up most of atom s volume
19 Mass Number (A) Total number of protons and neutrons Helps identify isotopes Mass # - Atomic # # of Neutrons
20 Isotopes Atoms of the same element that have different masses
21 The Isotopes of an element have Same chemical properties Different mass #s Same atomic # s and # p + Different # n o
22 Calculating the number of neutrons Mass # - Atomic # # of Neutrons Hyphen-notation Nuclear Notation Atomic mass Atomic # # Neutrons Example. Carbon C
23 Calculating the number of neutrons Mass # - Atomic # # of Neutrons Hyphen-notation Nuclear Notation Atomic mass Atomic # # Neutrons Example. Carbon C
24 Classwork - Isotopes Hyphen-notation Nuclear Notation Atomic mass Atomic # # Neutrons 1. Oxygen Silicon Phosphorus Nitrogen Neon Sodium-22
25 And now it s time for.. Mole calculations!!! Don t be afraid yet.
26 The Mole Be honest: Does this lab coat make me look fat? The mole is the SI unit for a large amount of something. 1. We have other units for amount e.g. pair, dozen, baker s dozen, etc. 2. How many items are in a mole? Introducing Avogadro s number atoms per mol 4. This number is so large it is pretty much only used for counting atoms and molecules e.g. 1 mol H 2 O has atom, i.e. 602,200,000,000,000,000,000,000 atoms
27 Each element has a unique molar mass Molar mass = mass of one mole of an element or compound. Units of measure: g/mol To find the molar mass of an element, look at its average atomic mass in the Periodic Table. Average atomic mass of Li = amu (per atom) Molar mass of lithium = g/mol (of atoms) This means that one atom of Li weighs amu And x atoms of Li weigh g!
28 1. Moles to Grams Equation #moles (mol) x molar mass (g/mol)
29 1. Moles to Grams - Example What is the mass in grams of 3.50 mol Cu? moles Cu grams Cu = grams Cu moles Cu g Cu 3.50 mol Cu = 1 mol Cu 222 g Cu
30 Moles to Grams: Practice Problems Book: p. 126 Practice problems on the bottom of the page, #1a-d 1. Write questions and answers 2. Show work 3. Write neatly; it s for a classwork grade!
31 2. Grams to Moles Equation Equation Mass (g) molar mass (g/mol) aka
32 2. Grams to Moles Sample Problem C A chemist produced 11.9 g of aluminum, Al. How many moles of aluminum were produced? grams Al moles Al grams Al = moles Al 1 mol Al 11.9 g Al = g Al mol Al
33 Grams to Moles: Practice Problems Add the following questions to your paper on moles to grams How many moles are in e. 650 g of Nitrogen f. 38 grams of Sulfur g. 12 grams of Carbon h. 890 g Oxygen 1. Write questions and answers 2. Show work 3. Write neatly; it s for a classwork grade!
34 Essential Questions - Section 4.3 Modern Atomic Theory 1. What is the modern model of the atom? 2. How does the modern atomic model differ from Rutherford s model of the atom? 3. How are the energy levels of an atom filled?
35 Section 4.3 Vocabulary Energy level Orbital S-orbital P-orbital
36 Modern Model of the Atom 1. Think as an atom as surrounded by concentric sphere. Each sphere is called an energy level.
37 Modern Model of the Atom 2. Electrons can be found only in certain energy levels, not between levels.
38 Modern Model of the Atom 3. Location of electrons cannot be predicted precisely (they are not in orbits, they are in clouds, which are called orbitals ).
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40 Modern Model of the Atom 4. Electrons must gain energy to move to a higher energy level or lose energy to move to a lower energy level. How do electrons gain energy? By getting zapped with light, electricity, heat, or any other kind of energy.
41 How many electrons does an element have? As many as the number of protons. which is the same as the atomic number. So if the atomic number is 4, then you have 4 protons and 4 electrons But you don t know how many neutrons you have!
42 Energy Levels 1. An area around the nucleus where electrons are located. 2. Each energy level may contain only a certain number of electrons.
43 How are the energy levels of an atom filled? 1. Depends on the number of electrons 2. Filled bottom up
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