Review before the quiz
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1 Do Now: Pick up sheets by the door (note packet and homework packet if you didn t pick one up last week) Take out completed homework #1 Take out Atoms Book
2 Review before the quiz 1) Bohr s model of the atom says that electrons a) are mixed in evenly with positive charge b) are found orbiting a positively-charged nucleus c) are found orbiting a positively-charged nucleus in energy levels (shells) d) are found in regions of probability around the nucleus called orbitals
3 Review Before the Quiz 5) Dalton s model of the atom states that atoms e) have positive particles called protons and negative particles called electrons f) have a positively-charged nucleus g) have a positively-charged nucleus with electrons in energy levels (shells) h) are hard solid indivisible spheres
4 Review Before the Quiz One model of the atom states that atoms are tiny particles composed of a uniform mixture of positive and negative charges. Scientists conducted an experiment where alpha particles were aimed at a thin layer of gold atoms. Most of the alpha particles passed directly through the gold atoms. A few alpha particles were deflected from their straight-line paths. (This question was taken directly from a Regents Exam).
5 Review before the quiz Most of the alpha particles passed directly through the gold atoms undisturbed. What does this evidence suggest about the structure of gold atoms? Atoms are mostly empty space
6 Review before the quiz A few of the alpha particles were deflected. What does this evidence suggest about the structure of the gold atoms? The nucleus must be positive since it deflects positively charged alpha particles
7 Quiz-E-Poo time 9.5 minutes Can use your notes/atom book. Turn ALL OF IT IN when you are done Atom Book Homework Quiz
8 Quiz Name Answers ¼ sheet of paper Name that model! 1) Atoms look like solid spheres 2) Atoms are mostly empty space 3)Electrons are found in distinct levels similar to the path of planets around the sun 4) The most up-to-date model 5) The first model to include electrons
9
10 Objective Describe the difference between a full and an occupied energy level What is an energy level? When is it full?
11 I. The Bohr Atom Bohr was the first to propose that the electrons were located in energy levels A lower case n is used to denote these principle energy levels (also called principle quantum numbers). The level closest to the nucleus is labeled n = 1. The next level is labeled n = 2 and so forth.
12 I. The Bohr Atom Each principle energy level had a certain energy value associated with the level. The closer the level was to the nucleus, the lower the energy of the level.
13 I. The Bohr Atom As long as the electrons were in these levels, the electrons do not give off energy.
14 Number the principle Energy levels
15 2. Electron Configuration and the Periodic Table Each principle energy level can only hold so many electrons before the level is full. A quick and easy way to determine the maximum number of electrons (max e - ) that a principle energy level can hold is given by the following:
16 max e - = 2 n 2. First square the principle energy level number (n) then multiply by 2
17 2n 2 Trick Principle Energy Level (n) Maximum Electrons
18 Electron Configuration Electrons are arranged around the nucleus by filling up the first principle energy level (n=1), then the second energy level, etc. (with some exceptions that we will get to later in the unit ) This is the electron configuration given on your periodic table.
19 Electron Configuration The number of electrons are listed for each level with a dash between levels: for oxygen (O) which has a total of 8 electrons, the configuration is 2 6
20 Electron Configuration 2 electrons are located in the first principle energy level 6 electrons are located in the second principle energy level.
21 Look up the electron config. on the PT for the element given & fill in the chart. Element n = 1 n = 2 n = 3 n = 4 Ca Na F B
22 Look up the electron config. on the PT for the element given & fill in the chart. Element n = 1 n = 2 n = 3 n = 4 Al C H
23 Side Bar: Look up # 72 Hf What does the ** mean? So the electron configuration of Hf is What is the electron configuration of gold (Au) # 79?
24 ADDITIONAL INFORMATION Ions: atoms with a charge because of gaining or losing an electron Gained an electron (-) charge Lost an electron (+) charge How would an Ion s configuration compare to a neutral atoms?
25 Ion Electron configuration Al Configuration : Al +3 Configuration: Na Configuration: Na +1 configuration: Cl configuration: Cl -1 configuration:
26 Ion Configuration Negative charge gained that many more electrons Positive charge lost that many electrons
27 Completely Filled vs. Occupied Principle Energy Levels Is this room occupied? Is this room filled?
28 Completely Filled vs. Occupied Principle Energy Levels Occupied means that there is at least one electron in the Principle Energy Levels (PEL) Li: 2 1 has 2 occupied PELs
29 Completely Filled vs. Occupied Principle Energy Levels Completely Filled means that each level has its maximum number of electrons which can be determined by the 2n 2 rule. n =1 then 2(1) 2 =2 & n = 2 then 2(2) 2 =8 Li: 2 1 has only 1 Completely Filled PEL
30 To help you review the 2n 2 rule complete the following chart PEL (n) Max e
31 In the chart: Copy the electron configuration from the Periodic Table Determine the number of Occupied Principle Energy Levels (PEL) Determine the number of Completely Filled Principle Energy Levels
32 Max e - : Elemen t Electron Conf. # ocup p # compl filled C
33 Max e - : Elemen t Electron Conf. # ocup p # compl filled Na O Cl
34 Max e - : Elemen t Electron Conf. # ocup p # compl filled He F Ne
35 Max e - : Elemen t Electron Conf. # ocup p # compl filled Si Zn Au
36 Ticket out How many full energy levels are there in an atom of Gold (Au)? Done: Do homework #2, all except the last problem
37 Do Now Take out your notes packet (page 4) Read how to draw bohr diagrams and attempt the first box (For F: Atomic # ) OBJECTIVE: Draw accurate bohr models of atoms
38 3. Drawing Bohr Diagrams of Atoms: 1) A circle is used for the nucleus- the # protons (# p or +) and the # of neutrons (#n) are placed in the circle. 2) A ring is drawn around the nucleus for each energy level. 3) The electrons for each energy level are placed in pairs symmetrically around the nucleus
39 For Fluorine (F) atomic # = atomic mass = electron configuration: # p = # n =
40 For Aluminum (Al) atomic # = atomic mass = electron configuration: # p = # n =
41 Going Backwards: Determining the identity of an element from the Bohr diagram: # p = # n = atomic # = atomic mass = # p + # n = electron configuration: Isotopic Notation:
42 Going Backwards: Determining the identity of an element from the Bohr diagram: # p = # n = atomic # = atomic mass = # p + # n = electron configuration: Isotopic Notation:
43 To review: To draw a Bohr Model: Look up the atomic #, atomic mass & the electron configuration Determine the # of neutrons (atomic massatomic #) Draw nucleus & write the # p & #n in nucleus Draw rings around the nucleus equal to the # of PEL in atom (# of numbers in electron configuration) Place electrons for each level symmetrically in the rings in pairs
44 Going Backwards writing Isotopic Notation: # of protons = atomic number so look up the atomic # to get symbol Add the # of protons and neutrons to get the atomic mass (mass #) Atomic mass is the top number Atomic # is the bottom number 10Ne 20
45 Now it is your turn! Complete the Bohr Model worksheet. When done, show me and turn in. If not done, it becomes homework along with homework #2.
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