Joke of the Day. Progress of the Atom. Discovering the Atom X X. CH 4- Atoms 1. Democritus Dalton Thomson. Rutherford X X Bohr X X X.
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1 Joke of the Day Discovering the Atom Progress of the Atom In this lesson we will take a look at the scientists who explored the wonders of the atom. QuickTime and a decompressor are needed to see this picture. Democritus Dalton Thomson Indivisible Electron Nucleus Orbit Electron Cloud X X Rutherford X X Bohr X X X Wave X X X X Elements of chemistry- Atoms, the building blocks of matter Video CH 4- Atoms 1
2 Timeline of Progress of the Atom What is in an Atom? Atoms are the building blocks of everything. Atoms can be divided, but not easily on Earth. Aristotle s 4 elements Nuclear Fission 118 different types of Atoms What is in an Atom? Parts of the Atom Particle Charge Mass (kg) Location Proton x In the nucleus Neutron x In the nucleus Electron x Outside the nucleus CH 4- Atoms 2
3 What is in an Atom? Contains: Proton, Electron, and Neutron Proton and neutron are 2000 times heavier than electron Mostly empty space No overall charge (Neutral) Same number of proton and electron only Protons How many protons? What is in an Atom? An element is defined by the number of protons Atomic Number NO TWO ELEMENTS WILL HAVE THE SAME NUMBER OF PROTONS. Positive (+) charge Located in the nucleus Electrons What is in an Atom? Neutrons What is in an Atom? Electron have a negative (-) charge Located outside the nucleus The electric force between protons in the nucleus and electrons outside the nucleus holds the atom together. Neutrons have no charge (0) and are neutral. Neutrons contribute to the atomic mass of the atom. 11 CH 4- Atoms 3
4 What is in an Atom? ELECTRON THE ATOM Contains the protons and neutrons Where most of the mass of the atom is concentrated Has an overall positive (+) charge PROTON THE NUCLEUS NEUTRON 13 Atomic Number and Mass Number Atomic number (Z) = the number of protons This is also the number of protons if the atom is neutral. No two elements share the same atomic number or number of protons 6 Carbon: Z = Hydrogen: Z = 1 Uranium: Z = 92 Atomic Number and Mass Number Mass number (A) = the total number of subatomic particles in the nucleus, that is the sum of the protons and the neutrons. Mass number is denoted by A Example: A fluorine atom has 9 protons and 10 neutrons, so A= 19 for fluorine. Carbon: A= 12 Chlorine: A= 35 Aluminum: A= 27 mass number can be estimated by rounding the average atomic mass. CH 4- Atoms 4
5 Finding # of Neutrons We can find the number of neutrons by subtracting the Atomic Number from the Mass Number. Mass number (A) -Atomic number (Z) Number of neutrons F has 10 neutrons. Al has neutrons = = 14 Joke for the Day Why shouldn t you trust an atom? They make up everything. Try this. Try This Identify the following two atoms Element Number of Protons Number of Neutrons Number of Electrons Atomic Mass Atomic Number A B Tantalum Radium Copyright 2010 Ryan P. Murphy CH 4- Atoms 5
6 Try This Atomic mass Average atomic mass (amu) is the weighted average of the masses of all the commonly occurring isotopes of an element. Ni= Fe= K= Copyright 2010 Ryan P. Murphy Ion Formation Atoms with a charge Different number of protons and electrons Form by changing the number of electrons ONLY It happens to atoms that do NOT have their outermost energy levels filled with electrons. EXAMPLE A neutral magnesium (Mg) atom has 12 protons and 12 electrons. If the magnesium atom loses 2 electrons, it will have a net electrical charge of 2. To find net charge of an ion, subtract the number of electrons from the number of protons. Number of protons = 12 - Number of electrons = A magnesium ion is represented as Mg +2. CH 4- Atoms 6
7 EXAMPLE 1: 1. Sodium (Na) atoms have 11 protons and electrons 11 with a net charge of If the Sodium ion only has 10 electrons, what is the net charge of the ion?. ( = +1) 3. What is the chemical symbol for this ion? Na +1 EXAMPLE 2: 1. Beryllium (Be) atoms have 4 protons and electrons 4 with a net charge of If the Beryllium ion has only 2 electrons, what is the net charge of the ion?. (+4-2 = +2) 3. What is the chemical symbol for this ion? Be 2+ Learning Check Counting Learning Check State the number of protons, neutrons, and electrons in each of these ions. 39 K + 16 O Ca #p #n o #e Write the nuclear symbol form for the following atoms or ions: A. 8 p +, 8 n, 8 e - B. 17p +, 20n, 17e - C. 47p +, 60 n, 46 e - O Cl Ag + CH 4- Atoms 7
8 An isotope is an atom that has the same number of protons but a different number of neutrons (relative to other atoms of the element). Same number of electrons They vary in mass and mass number (A). A - Z = n Isotopes 6n How many Neutrons? Atomic number stays the same. Why? Same number protons 8n What are Isotopes? All atoms of an element have the same atomic number and the same number of protons. However, atoms do not necessarily have the same number of neutrons. Atoms with the same number of electrons and protons, but different numbers of neutrons, are called isotopes. Different isotopes belong to the same element because they have the same number of electrons, which means that they all behave almost the same in chemical reactions. Same element, but different mass due to different number of neutrons. Carbon-12 Isotopes Both Carbon Carbon-14 Isotopes CHANGE IN WEIGHT, BUT NOT CHARGE TWO ISOTOPES OF HYDROGEN. ON THE LEFT, ONE NEUTRON ON THE RIGHT, THERE ARE TWO NEUTRONS 6 PROTONS 6 PROTONS 8 NEUTRONS CH 4- Atoms 8
9 Isotopes Atoms of the same element (same Z) but different mass number (A). Boron-10 ( 10 B) has 5 p and 5 n Boron-11 ( 11 B) has 5 p and 6 n 10 B 11 B Isotopes of Hydrogen Hydrogen 1 Protons = 1 Electrons = 1 Neutrons = 0 Hydrogen 2 Protons = 1 Electrons = 1 Neutrons = 1 Hydrogen 3 Protons = 1 Electrons = 1 Neutrons = 2 Isotopes? Which of the following represent isotopes of the same element? Which element? 234 X 234 X 235 X 238 X Isotope Neptunium Isotope Uranium Learning Check Counting Naturally occurring carbon consists of three isotopes, 12 C, 13 C, and 14 C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12 C 13 C 14 C #p #n o #e CH 4- Atoms 9
10 Complete Nuclear Symbols Practice Problems Isotopes should be written using the complete nuclear symbol or by using a hyphen symbol. A charge should be indicated if the atom is not neutral. EXAMPLE: (hyphen symbol) Chlorine - 37 mass number Complete nuclear symbol for an element is written like this mass number atomic number Cl +2 element symbol and charge 1. List out the number of protons, electrons, and neutrons of Pb 2. List out the number of protons, electrons, and neutrons of Atoms of a certain isotope have 73 neutrons and a mass of 123. a. What is the atomic number? 25 Mn +2 b. How many electrons are there? c. What is the name of the element? d. Write the chemical symbol for this isotope. CH 4- Atoms 10
11 Learning Check Moles Molecular Weight Molecular Mass Formula Weight Formula Mass An atom has 14 protons and 20 neutrons. A. Its atomic number is 1) 14 2) 16 3) 34 B. Its mass number is 1) 14 2) 16 3) 34 C. The element is 1) Si 2) Ca 3) Se D. Another isotope of this element is 1) 34 X 2) 34 X 3) 36 X Molar mass: the mass, in grams, of one mole of a substance. Avogadro s number: X This is defined as the number of particles in 12 g of Carbon-12. Avogadro s number is not useful for larger objects x 10²³ Amedeo Avogadro The Mole! 602,213,670,000,00 0,000,000,000 particles! CH 4- Atoms 11
12 Modern Atomic Theory Electrons can be found only in certain energy levels, not between levels. Electron location (not precise) is limited to energy levels. Energy Level Describe the path the electron takes around the nucleus Farther from nucleus is more energy Gain energy they move away (absorbing photon) Lose energy they move toward (release photon) Only certain energies are allowed in each atom Bohr Model Bohr models show every electrons on each energy level of an atom. Energy Levels Like an elevator it can only be on certain floors Never in between Energy levels get closer together the higher you go Each has room for a certain number of electrons Argon-18 4 th Energy Level 3 rd Energy Level 8e - 2 nd Energy Level 8e - 1 st Energy Level 2e - Nucleus CH 4- Atoms 12
13 Electron structure Consider an atom of Potassium Nucleus The inner shell has electrons The next shell has electrons The next shell has electrons The next shell has the remaining electron Electron structure = 2,8,8,1 Regions where you have a chance of finding the electron There are different types of orbitals s, p, d, f Orbitals Each has its own shape or shapes Each shape has room for two electrons Each can be found in the energy levels S orbital P orbital 3 dumbbell-shaped regions Each p orbital can hold a maximum of 2 electrons, so all three together can hold a total of 6 electrons. CH 4- Atoms 13
14 d orbital Five different shapes More complex Each can hold 2 electrons Total of 10 electrons f orbital seven different shapes Much more complex Each can hold 2 electrons Total of 14 electrons CH 4- Atoms 14
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