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Atomic structure
My report on "Atomic Structure"
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Page 1 : http://mw2.concord.org/public/part2/atomstrk/page1.cml
1. Now imagine that some random person walks up and throws one dart at the board. Based on the pattern of holes you've seen from previous players, where will this dart most likely land: hint
(a) There is no way to tell.
(b) Close to the center of the board.
(c) Out toward the edge of the board.
My answer is (b) (6:30:39 PM)
2. Explain the reasoning behind your prediction:
It is based on probability. If previously, the majority of the darts hit close to the centre,(based on chance) that's where most of the following darts will hit. The same concept is utilized for stock analysis; if a corporation is on the rise, the notion would be to remain bull and buy rather than sell. (6:34:32 PM)
Page 2 : http://mw2.concord.org/public/part2/atomstrk/page2.cml
1. Explain why the color of the orbital gets lighter as you move further from the nucleus: (see completed orbital above and to the right)
The colour of the orbital gets lighter as you move further from the nucleus because there is less overlap at this distance. The electrons are present around the nucleus, and show up more frequently closer to the nucleus. This means that when you trace the location of the electrons, you see a darker shade in the centre and lighter farther away. An electron has less liklihood to appear on the outer limits of it's orbit, than it does within (where density is greater). (6:40:22 PM)
2. If you had to bet on where you are most likely to find an electron at any particular point in time, where would it be?
(a) Near the nucleus.
(b) Away from the nucleus.
(c) There is a perfectly even chance of finding an electron anywhere.
My answer is (a) (6:40:04 PM)
Page 3 : http://mw2.concord.org/public/part2/atomstrk/page3.cml
1. Which sub-atomic particle defines the kind of element an atom will be? hint
(a) electron
(b) proton
(c) neutron
My answer is (b) (6:52:25 PM)
2. Which number defines the kind of element an atom will be?
(a) mass number
(b) atomic number
(c) a combination of both mass and atomic number
My answer is (b) (6:52:43 PM)
3. Explain how you can predict the atomic number and the mass number by using an atom's number of protons and/or neutrons.
Since the atomic number represents the number of protons an atom has, then this direct correlation can easily be seen.
The number of electrons can be determined via the atomic and mass number. The mass number of an atom is the total number of neutrons and protons. By taking the mass number and subtracting the atomic number we can retreive the number of neutrons (Mass # - Atomic # = Neutrons). (6:58:02 PM)
4. Put a snapshot of your lithium atom here.
Lithium atom created by increasing the mass number to 3. (6:53:44 PM)
Page 4 : http://mw2.concord.org/public/part2/atomstrk/page4.cml
1. What would be the charge on an atom with 7 protons and 4 electrons?
+3 (6:59:26 PM)
2. What would be the charge on an atom with 7 protons and 8 electrons?
-1 (6:59:44 PM)
3. An atom is NOT an ion when:
(a) there are no electrons
(b) there are an equal number of protons and electrons
(c) the number of protons and neutrons cancel out
(d) the atom has no overall charge
(e) both B and D
My answer is (e) (6:59:48 PM)
4. Explain how can you predict the overall charge by knowing an atom's number of protons and electrons.
Protons are the positive subatomic particle that comprises an atom. For every one proton present, the charge increases by +1.
Electrons are the fundamental particles of an atom that contains a negative charge. For every one electron present, the charge is altered by -1.
Therefore, the charge can be determined by the relationship:
# of Protons - # of Electrons = Overall Charge (7:03:05 PM)
Page 5 : http://mw2.concord.org/public/part2/atomstrk/page5.cml
1. What is different and what is the same between these carbon isotopes? (check all that apply)
(a) the mass number is the same
(b) the atomic number is the same
(c) the mass number is different
(d) the atomic number is different
(e) the number of protons is the same
(f) the number of protons is different
(g) the number of neutrons is the same
(h) the number of neutrons is different
My answer is (b) (c) (e) (h) (7:09:19 PM)
2. Scientists use the fact that living things have a lot of carbon in them. When they die the radioactive isotope breaks down over time, turning into other elements. By seeing how much of the radioactive carbon is left you can tell how old something is. Which one of these isotopes of carbon is radioactive, and can be used for carbon dating?
(a) carbon-12
(b) carbon-13
(c) carbon-14
My answer is (c) (7:09:37 PM)
3. Try making several stable and radioactive forms of other elements. What is the general rule for creating an atom with a stable nucleus (one that is NOT radioactive)?
As you alter the atomic number (amount of protons), in order to regenerate a stable nucleus you must increase the amount of neutrons as well. In some cases, the same number of both protons and neutrons can cause the atom to be radioactive, but generally as long as there are as many neutrons as protons, the atom will remain stable. Although this rule is merely general, you can add additional neutrons to change the mass number of the isotope. Adding more than 1-2 neutrons causes radioactivity though. (7:18:28 PM)
Page 6 : http://mw2.concord.org/public/part2/atomstrk/page6.cml
1. Click on the energy diagram to determine which orbital this is, and record the name of the orbital below:
3d (7:23:44 PM)
2. Electron orbitals (choose all that are correct):
(a) get bigger at higher energies
(b) get smaller at higher energies
(c) stay about the same size regardless of energy
My answer is (a) (7:23:47 PM)
Page 7 : http://mw2.concord.org/public/part2/atomstrk/page7.cml
1. In what order do electrons form boron’s orbitals?
(a) from lowest energy to highest
(b) from highest energy to lowest
(c) they randomly form various orbitals
My answer is (a) (7:28:18 PM)
2. Which orbital is the one that would give the best estimate of the size of this atom?
(a) 1s
(b) 2s
(c) 2p
My answer is (b) (7:28:42 PM)
3. Take a snapshot of the boron atom showing all the overlapping orbitals.
(7:29:57 PM)
Page 8 : http://mw2.concord.org/public/part2/atomstrk/page8.cml
1. What happens to the size of an atom as you go across the table from left to right. Pick a row (also called a period) and click on each atom, starting from the left.
(a) the atoms get bigger
(b) the atoms get smaller
(c) the atoms stay the same size
(d) the size changes randomly
My answer is (b) (7:31:56 PM)
2. What happens to the size of an atom as you go down a column. Pick a column (also called a group) and click on each atom, starting from the top.
(a) the atoms get bigger
(b) the atoms get smaller
(c) the atoms stay the same size
(d) the size changes randomly
My answer is (a) (7:32:16 PM)
Page 9 : http://mw2.concord.org/public/part2/atomstrk/page9.cml
From this 2D image, it appears the number of protons and neutrons are the same.
This atom has the same amount of neutrons and protons.
1. What is an orbital? Describe in detail.
An orbital is the region surrounding the nucleus of an atom where electrons are more likely to be found. These orbitals can also be defined as the different quantum states in which electrons may be found.
The primary quantum position is indicated by an "s", and is where the first two electrons of an atom lie (as indicated from page 7's tutorial regarding Boron). Subsequent quantum states are indicated by differing letters. (7:57:36 PM)
2. What would be the charge of an ion with 10 protons and 12 electrons?
(a) it would be neutral
(b) +2
(c) -2
(d) 22
(e) 10
My answer is (c) (7:50:15 PM)
3. What is true when comparing these two isotopes? (check all that apply)
(a) they have the same number of protons
(b) they have the same number of neutrons
(c) both are have a -4 charge
(d) they are different elements
(e) they are both likely to be radioactive
My answer is (b) (d) (7:54:45 PM)
4. To the right you see part of a periodic table that shows the sizes of the atoms. Describe why it makes sense to start a new row with Li, and then another with Na:
It makes sense to create a new row with Li, and Na, in the periodic table of the elements because of the size of the atoms. For sheer means of simplicity and generating a pattern, the table was set up as displayed. Also, the valence electrons in the coloums line up according to quantity. For example, Li and Na have 1 electron in their electron shell. Be and Mg have 2, and so on down the table. If Li continued after Ne, it wouldn't correlate effectively with hydrogen or sodium which share this exact number of valence electrons. (8:05:34 PM)
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