Bell Ringer: How do you know something exists if you have never seen it before? Important Vocabulary Inference Indirect evidence Nature of Science
Dec 25, 2015
Bell Ringer: How do you know something exists if you have never seen it before?
Important Vocabulary
Inference
Indirect evidence
Nature of Science
The Black Box Lab
Purpose Materials Procedure Results Table (20 pts)Post Lab Questions (30 pts)
Results (20 pts)
Box # Inferences Model
Example
a)
b)
c)
1
a)
b)
c)
Post Lab Questions (30pts)
1. How did you construct your model of what was in the boxes?
2. How do you know if something exists if you have never seen it before?
3. How does this lab relate to the scientific method?
4. To create a more accurate model, what would you want to do next without looking inside the boxes?
5. How do you think scientists use or have used empirical evidence to create models? (hint: think about topics in this class)
Contents of Each Box
• Box 1- Wooden block
• Box 2 - 3 Pennies
• Box 3 - 2 Straws
• Box 4 - 10 Stickers
• Box 5 - Pill Canister
• Box 6 – 2 Rubber bands
• Box 7 - 1 Dice
• Box 8- 10 Beads
• Box 9 - 10 Lima Beans
• Box 10 - 2 Cotton Balls
Closure: watch video “have you ever seen an atom?”
Exit Pass – how does today’s lab relate to the discovery of the atom?
What does an atom actually look like?
It is now your turn to do some research…
You will be assigned a scientist to become an expert on
This scientist had an impact on the historical development of the atom
YOUR JOB: give a creative, informative poster on your scientist and how they influenced the historical development of the atom
You are then going to share your poster with others to inform them about your scientist.
Historical Scientists Jigsaw Activity
Textbook Info
Dalton – pg 77-78
Thomson – pg 79
Rutherford – pg 81
Bohr – pg 91
DeBroglie – pg 91
Atoms
New section in table of contents
Aristotle & Democritus
First philosophers to start thinking about the atom and its component
Smallest divisible component vs. indivisible particle
Dalton
Billiard Ball Model
Provided evidence for how we know atoms exist
EQ 1: How do we know atoms exist?
KC 1: Law of definite proportions – a chemical compound always contains the same elements in exactly the same proportions by weight or mass
KC 2: Law of conservation of mass
KC 3: Law of multiple proportions – when 2 elements combine to form 2 or more compounds, the mass of one element that combines with a given mass of the other is in the ratio of small whole numbers
EQ 2: What are the five postulates of Dalton’s atomic theory
The ancient Greeks tried to explain matter, but the scientific study of the atom began with John Dalton in the early 1800's.
KC 1: All matter is composed of extremely small particles called atoms, which cannot be subdivided, created, or destroyed
Many ancient scholars believed matter was composed of such things as earth, water, air, and fire.
Many believed matter could be endlessly divided into smaller and smaller pieces
EQ 2: What are the five postulates of Dalton’s atomic theory
KC 2: Atoms of a given element are identical in their physical and chemical properties
KC 3: Atoms of different elements differ in their physical and chemical properties
EQ 2: What are the five postulates of Dalton’s atomic theory
KC 4: Atoms of different elements combine in simple, whole-number ratios to form compounds
KC 5: In chemical reactions,
atoms are combined,
separated, or rearranged
but never created,
destroyed, or changed
EQ 2: What are the five postulates of Dalton’s atomic theory
Thomson
Plum pudding model
Introduced the idea that electrons are located outside the nucleus
Rutherford
Discovered the nucleus
Used the gold foil experiment
EQ 3: What model of the atom will we use?
KC 1: Bohr suggested that electrons move in circular orbitals around the nucleus
Bohr’s model of the atom gives us a good starting point for understanding more about the atom
EQ 3: What model of the atom will we use?
KC 2: How to draw a Bohr model of an atom
1) Find your element on the periodic table.
2) Determine the number of electrons – it is the same as the atomic number.
3) Determine the number of circular orbits the atom has.
4) Add electrons = atomic number
- 1st shell can hold two
- 2nd and 3rd can hold eight
Bohr model of the atom
Elements in the 1st period have one energy level.
Elements in the 2nd period have two energy levels, and so on.
C
Bohr model of the atom
Draw a nucleus with the element symbol inside.
Carbon is in the 2nd period, so it has two energy levels, or shells.
Draw the shells around the nucleus.
Bohr model of the atom
Element name
Atomic number = number of protons = number of electrons (for now…)
Element symbol
Average atomic mass
C
Bohr model of the atom
Add the electrons.
Carbon has 6 electrons.
The first shell can only hold 2 electrons.
C
Bohr model of the atom
Since you have 2 electrons already drawn, you need to add 4 more.
These go in the 2nd shell.
Add one at a time -starting on the right side and going counter clock-wise.
C
Bohr model of the atom
Check your work. You should have 6 total
electrons for Carbon. Only two electrons can
fit in the 1st shell. The 2nd shell can hold up
to 8 electrons. The 3rd shell can hold 18,
but the elements in the first few periods only use 8 electrons.
Bohr model of the atom
KC 3: The lowest allowable energy state of an atom is called its ground state.
KC 4: When an atom gains energy, it is in an excited state.
Wavelike properties of electron help relate atomic emission spectra, energy states of atoms, and atomic orbitals
Bohr model of the atom
A photon is a particle of electromagnetic radiation having zero mass and carrying a quantum of energy.
When a photon strikes an atom it gives the atoms more energy. If enough photons strike an atom it may cause electrons to jump levels.
Bohr model of the atom
KC 5: The excited state occurs when an atom has a higher potential energy than it has at its ground state.
When an excited atom falls back to its ground state the substance will give off a unique color of light.
Bohr model of the atom
KC 6: The behavior of electrons is still not fully understood, but it is known that they do not move around the nucleus in circular orbits
We use Bohr’s model because it is easy to picture and gives us a basic understanding of the atom
Whiteboard Practice
Draw the Bohr model for the following elements:Boron
Calcium
Chlorine
Nitrogen
EQ 4: What is an atom made of?
Know Want to know Learned
EQ 4: What is an atom made of?
KC 1: An atom is made of a nucleus containing protons and neutrons. Electrons move around the nucleus.
EQ 4: What is an atom made of?
KC 2: The number of protons and the mass number define the identity of the atom
Each element contains a unique positive charge in their nucleus
What is an atom made of?
KC 3: The number of protons in the nucleus of an atom identifies the element and is known as the element’s atomic number
Atoms and Isotopes
All atoms of a particular element have the same number of protons and electrons but the number of neutrons in the nucleus can differ
KC 4: Atoms with the same number of protons but different numbers of neutrons are called isotopes
Atomic Mass and Isotopes
The relative abundance of each isotopes is usually constant
Isotopes containing more neutrons have a greater mass
Isotopes have the same chemical behavior
KC 5: The atomic mass is the sum of the protons and neutrons in the nucleus
Atomic Mass and Isotopes
Isotopes
There are 2 ways you will see isotopes written:
Aluminum-27
Al2713
One atomic mass unit (amu) is defined as 1/12th the mass of a carbon-12 atom
One amu is nearly, but not exactly, equal to one proton and one neutron.
Atomic Mass
Calculating Averages
If you are shopping, and something is $24.99 and 15% off, how much would you pay?
Average Atomic Mass
KC 6: The average atomic mass of an element is the weighted average mass of the isotopes of that element
Average Atomic Mass
Average atomic mass = (mass1 x abundance1) + (mass2 x abundance2) + …
Istotope Mass Abundance Total
Mg - 24 23.985 0.7870 18.876
Mg - 25 24.986 0.1013 2.531
Mg - 26 25.983 0.1117 2.902
Average atomic mass = 24.309 amu
Practice Problems
1. The four isotopes of lead and its abundances are: Pb-204, 1.37%; Pb-206, 26.26%; Pb-207, 20.82%; and Pb-208, 51.55%. Calculate lead’s approximate atomic mass.
Istotope Mass Abundance Total
Pb-204
Pb-206
Pb-207
Pb-208
Average atomic mass =
Practice Problems
2. Calculate the average atomic mass of neon if neon exists naturally as 90.92% neon-20, 0.257% neon-21, and 8.82% neon-22.
Istotope Mass Abundance Total
Average atomic mass =
Practice Problems
3. Titanium has 5 common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%), 49Ti (5.5%), 50Ti (5.3%). What is the average atomic mass of titanium?
EQ 5: How do you determine the number of protons, neutrons, and electrons in an atom?
Atom Basics – building blocks of chemistry These are must knows!!
You must be able to answer the following questions…
1. What is my name?
2. What is my atomic number?
3. What is my average atomic mass?
4. (Pick one of my isotopes on the left side of the card). What would the atomic mass of that particular atom?
5. How many protons do I have?
6. How many neutrons do I have?
7. How many electrons do I have if I am neutral?
8. (Pick an ion of the right side of the card). How many protons and electrons do I have?
9. (Consider that I am the previous chosen isotope above and a neutral atom) What happens to me if I gain a
p+_________ no_________ e- ________
10. What happens to me if I lose a
p+_________ no_________ e- _________
1. What is my name?
2. What is my atomic number?
KC 1: An atom’s atomic number is equal to the number of protons, which is found on the periodic table
3. What is my average atomic mass?
KC 2: Average atomic mass is the averages of all of the isotopes of an element. This number is calculated and based on abundance, but also found on the periodic table.
4. What is the atomic mass of a particular isotope?
5. How many protons do I have?
KC 3: The number of protons is equal to the atomic number, which is found on the periodic table
6. How many neutrons do I have?
KC 4: The atomic mass = protons + neutrons
Atomic number = number of protons
KC 5: neutrons = atomic mass – atomic number
7. How many electrons do I have if I am neutral?
KC 6: The number of electrons is equal to the number of protons in a neutral atom
8. How many protons and neutrons do I have if I am neutral?
If the atom is neutral, the protons and neutrons are found from the atomic mass and atomic number of that particular isotope
Protons = atomic number
Neutrons = atomic mass – atomic number
9. & 10. What happens if I gain/lose a p+, n0, and e-?
KC 7: When the number of protons changes, the identity of the element changes
KC 8: When the number of neutrons changes, the atomic mass changes
KC 9: When the number of electrons changes, the atom is no longer neutral and has a charge
What happens if I gain/lose a p+, n0, and e-?
Example: Calcium – 40
p+________________ no________________ e- _________________
1. What is my name?
2. What is my atomic number?
3. What is my average atomic mass?
4. (Pick one of my isotopes on the left side of the card). What would the atomic mass of that particular atom?
5. How many protons do I have?
6. How many neutrons do I have?
7. How many electrons do I have if I am neutral?
8. (Pick an ion of the right side of the card). How many protons and electrons do I have?
9. (Consider that I am the previous chosen isotope above and a neutral atom) What happens to me if I gain a
p+_________ no_________ e- ________
10. What happens to me if I lose a
p+_________ no_________ e- _________