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29 Cards in this Set
- Front
- Back
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How many electrons are there in: 23 NA ? 11
What do the top and bottom numbers represent? |
11 electrons 11 protons 12 neutrons
The 23 is the atomic mass (protons and neutrons). The 11 is the atomic number (protons) |
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How many electrons are there in: 19 F ? 9
What do the top and bottom numbers represent? |
9 electrons 9 protons 10 neutrons
The 19 is the atomic mass (protons and neutrons). The 9 is the atomic number (protons) |
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What is an ISOTOPE? |
Atoms of the same element that have different numbers of neutrons. |
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What is the isotopic name of 12 C 6 |
Carbon-12 |
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What is the atomic mass, number of protons, and number of electrons of boron-11? |
Atomic mass = 11 Atomic number (protons) = 5 Electrons = 5 |
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Calculate the average atomic mass of silicon-28 assuming a mass of 27.977 and abundance of 92.21%. |
27.977 x 0.9221 = 25.80 |
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What are the different energy sublevels? |
s, p, d, f |
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What is the maximum number of electrons in sublevel s? |
2 electrons |
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What is the maximum number of electrons in sublevel p? |
6 electrons |
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What is the maximum number of electrons in sublevel d? |
10 electrons |
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What is the maximum number of electrons in sublevel f? |
14 electrons |
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How many energy sublevels are there at energy level 2? What are they? |
Two: 2s, 2p |
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How many energy sublevels are there at energy level 3? What are they? |
Three: 3s, 3p, 3d |
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How many energy sublevels are there at energy level 4? What are they? |
Four: 4s, 4p, 4d, 4f |
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What is the maximum number of electrons possible in energy level 4? |
s (2) + p (6) + d (10) + f (14) = 32 electrons |
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What is the electronic configuration of Mg? |
Mg has 12 electrons: 1s(2), 2s(2), 2p(6), 3s(2) |
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Where would you be highly likely to find an electron? |
The atomic orbital |
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When using the periodic table to determine electronic configuration, what is unique about using the "D" block to identify electron sublevels? |
The "D" block always "back-fills" to the previous main energy level (this avoids the ordering problem for most elements). |
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When using the periodic table to determine electronic configuration, what is unique about using the "F" block to identify electron sublevels? |
The "F" block always "back-fills" twice to two main energy levels before the current main energy level (this avoids the ordering problem for most elements). |
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Write the electron configuration of Rn. |
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2,4d10, 5p6, 6s2, 4f14, 5d10, 6p6 |
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What equation represents the max number of electrons that can occupy an energy level (n)? |
2n^2 |
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An element with the outermost electron configuration of ns2np4 would be in Group:? |
VIB |
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How many electrons are in the outermost shell of a Group VIIB element? |
7 |
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What would be the outer electron configuration of group VIB? |
ns2, np4 |
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Atomic radius ________ as you move left to right across a period (row) on the periodic table. |
DECREASES |
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Atomic radius generally _________ as you move down a group (column) on the periodic table. |
INCREASES |
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The minimum energy required to remove the most loosely held electron is __________. |
"first ionization energy" |
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First ionization energy (potential) generally ________ as you move down a group (column) on the periodic table. |
DECREASES |
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The amount of energy given off in the process in which an electron is added to a neutral gaseous atom is defined as _____________. |
"electron affinity" |
