section #1: history of the periodic table
1) who is attributed with the idea of arranging the known elements of his time in a table according to their chemical and physical properties? ______
2) this scientist from question #1, above, predicted that the empty spaces on his periodic table represented
a) radioactive elements. c) undiscovered elements.
b) isotopes. d) ions.
3) who arranged the periodic table of elements in the order of atomic number? ______
4) the periodic law states there is a periodic repetition of physical and chemical properties of the elements
a) when they are arranged in order of increasing atomic radii.
b) if only nonmetals are considered.
c) when they are arranged in order of increasing atomic mass.
d) when they are arranged in order of increasing atomic number.

section #2: the periodic table
5) the vertical columns of the periodic table are called ____________.
6) each period in the periodic table corresponds to ____________.
a) a sublevel c) an energy level
b) atomic mass d) an atomic number
7) what are valence electrons? ______
8) the horizontal rows of the periodic table are called ____________.
9) what do elements in the same periodic group have in common? ______
10) what do elements in the same periodic periods have in common? ______
11) how many elements are in a period in which only the s and p sublevels are filled? ______
12) identify the sublevels in a period that contains 32 elements.
a) s, d b) s, p c) s, p, d d) s, p, d, f
13) the number of valence electrons in group 17 elements is ____________.
14) for groups 13 through 18, the number of valence electrons is equal to ____________.
15) for group 2 elements, which sublevel are the valence electrons located in? ____________.

section #3: elements classes and families
16) name the three classes of elements. ______
17) identify the following on the periodic table to the right.
a). ____________
b). ____________
c). ____________
(image of periodic table with a, b, c marked)
18) name the element:
a) period 5, group 14 ______
b) period 3, group 17 ______
c) period 6, group 2 ______

Question

section #1: history of the periodic table
1) who is attributed with the idea of arranging the known elements of his time in a table according to their chemical and physical properties? ______
2) this scientist from question #1, above, predicted that the empty spaces on his periodic table represented
   a) radioactive elements.  c) undiscovered elements.
   b) isotopes.            d) ions.
3) who arranged the periodic table of elements in the order of atomic number? ______
4) the periodic law states there is a periodic repetition of physical and chemical properties of the elements
   a) when they are arranged in order of increasing atomic radii.
   b) if only nonmetals are considered.
   c) when they are arranged in order of increasing atomic mass.
   d) when they are arranged in order of increasing atomic number.

section #2: the periodic table
5) the vertical columns of the periodic table are called ____________.
6) each period in the periodic table corresponds to ____________.
   a) a sublevel  c) an energy level
   b) atomic mass d) an atomic number
7) what are valence electrons? ______
8) the horizontal rows of the periodic table are called ____________.
9) what do elements in the same periodic group have in common? ______
10) what do elements in the same periodic periods have in common? ______
11) how many elements are in a period in which only the s and p sublevels are filled? ______
12) identify the sublevels in a period that contains 32 elements.
    a) s, d  b) s, p  c) s, p, d  d) s, p, d, f
13) the number of valence electrons in group 17 elements is ____________.
14) for groups 13 through 18, the number of valence electrons is equal to ____________.
15) for group 2 elements, which sublevel are the valence electrons located in? ____________.

section #3: elements classes and families
16) name the three classes of elements. ______
17) identify the following on the periodic table to the right.
    a). ____________
    b). ____________
    c). ____________
    (image of periodic table with a, b, c marked)
18) name the element:
    a) period 5, group 14 ______
    b) period 3, group 17 ______
    c) period 6, group 2 ______

Accepted Answer

### Question 1
# Brief Explanations:
Dmitri Mendeleev is credited with arranging known elements in a table by their chemical and physical properties.
# Answer:
Dmitri Mendeleev

### Question 2
# Brief Explanations:
Mendeleev's empty spaces in his periodic table were predictions of undiscovered elements (e.g., he predicted gallium, scandium, germanium). Radioactive elements, isotopes, and ions don't fit the context of empty spaces in his table.
# Answer:
c) undiscovered elements

### Question 3
# Brief Explanations:
Henry Moseley arranged the periodic table by atomic number (the number of protons in an atom), which fixed inconsistencies in Mendeleev's table (arranged by atomic mass).
# Answer:
Henry Moseley

### Question 4
# Brief Explanations:
The periodic law states that when elements are arranged in order of increasing atomic number, their physical and chemical properties repeat periodically. Atomic radii order, nonmetals only, or atomic mass order (Mendeleev's original, with inconsistencies) don't define the modern periodic law.
# Answer:
d) when they are arranged in order of increasing atomic number

### Question 5
# Brief Explanations:
Vertical columns in the periodic table are called groups (or families). They share similar chemical properties due to the same number of valence electrons.
# Answer:
groups (or families)

### Question 6
# Brief Explanations:
Each period (horizontal row) corresponds to an energy level (principal quantum number, $ n $). Sublevels are within energy levels, atomic mass and number don't define periods this way.
# Answer:
c) an energy level

### Question 7
# Brief Explanations:
Valence electrons are the electrons in the outermost energy level (valence shell) of an atom. They determine an element's chemical reactivity and bonding behavior.
# Answer:
Electrons in the outermost energy level of an atom

### Question 8
# Brief Explanations:
Horizontal rows in the periodic table are called periods. Elements in a period have electrons filling the same energy level (e.g., period 1: $ n = 1 $, period 2: $ n = 2 $, etc.).
# Answer:
periods

### Question 9
# Brief Explanations:
Elements in the same group (vertical column) have the same number of valence electrons. This gives them similar chemical properties (e.g., group 1: 1 valence electron, reactive metals; group 17: 7 valence electrons, reactive nonmetals).
# Answer:
Same number of valence electrons (and similar chemical properties)

### Question 10
# Brief Explanations:
Elements in the same period (horizontal row) have electrons in the same energy level (same principal quantum number, $ n $). For example, period 3 elements have electrons in $ n = 3 $ (3s, 3p, and 3d for transition metals, but main - group elements use 3s and 3p).
# Answer:
Same energy level (same principal quantum number for electrons)

### Question 11
# Brief Explanations:
1. The $ s $ sublevel can hold 2 electrons, and the $ p $ sublevel can hold 6 electrons.
2. To find the number of elements in a period with only $ s $ and $ p $ sublevels filled, we add the number of electrons in $ s $ and $ p $ sublevels: $ 2 + 6=8 $.
# Answer:
8

### Question 12
# Brief Explanations:
1. The $ s $ sublevel holds 2, $ p $ holds 6, $ d $ holds 10, and $ f $ holds 14 electrons.
2. For a period with 32 elements, we need to sum the electrons in $ s $, $ p $, $ d $, and $ f $ sublevels: $ 2 + 6+10 + 14 = 32 $. So the sublevels are $ s $, $ p $, $ d $, $ f $.
# Answer:
d) $ s, p, d, f $

### Question 13
# Brief Explanations:
Group 17 elements (halogens) have 7 valence electrons. The group number (17) for main - group elements (excluding transition metals) can be related to valence electrons: for groups 1 - 2, it's the group number; for groups 13 - 18, it's group number - 10. So $ 17-10 = 7 $.
# Answer:
7

### Question 14
# Brief Explanations:
For main - group elements in groups 13 through 18, the number of valence electrons is equal to the group number minus 10. For example, group 13 has 3 valence electrons ($ 13 - 10 = 3 $), group 14 has 4, etc.
# Answer:
the group number minus 10 (or equal to the group number for 13 - 18: group 13 = 3, group 14 = 4, ..., group 18 = 8)

### Question 15
# Brief Explanations:
Group 2 elements (alkaline earth metals) have valence electrons in the $ s $ sublevel. Their electron configuration ends with $ ns^{2} $, where $ n $ is the period number. So the valence electrons are in the $ s $ sublevel.
# Answer:
$ s $ sublevel

### Question 16
# Brief Explanations:
The three classes of elements are metals (good conductors, malleable, ductile), nonmetals (poor conductors, brittle), and metalloids (properties between metals and nonmetals, semiconductors).
# Answer:
Metals, Nonmetals, Metalloids

### Question 17 (assuming the diagram: A is a transition metal, B is a nonmetal, C is a noble gas or another nonmetal region)
# Brief Explanations:
- A: Likely a transition metal (located in the d - block, middle of the periodic table).
- B: Likely a nonmetal (e.g., in the p - block, right - hand side, not noble gas).
- C: Likely a noble gas (group 18, far right) or another nonmetal. (Exact identification depends on the diagram, but general regions: A - transition metals, B - nonmetals (e.g., halogens or chalcogens), C - noble gases or other nonmetals)
# Answer:
- A: Transition Metal (e.g., if A is in the d - block)
- B: Nonmetal (e.g., Halogen or Chalcogen)
- C: Noble Gas (or other Nonmetal, depending on position)

### Question 18
#### Part a
# Brief Explanations:
1. Period 5 means the 5th energy level ($ n = 5 $), group 14 means 4 valence electrons (group 14: $ 14 - 10 = 4 $).
2. The element in period 5, group 14 is tin (Sn). Its electron configuration is $ [Kr]4d^{10}5s^{2}5p^{2} $, and it's in period 5 (row 5) and group 14 (column 14).
# Answer:
Tin (Sn)

#### Part b
# Brief Explanations:
1. Period 3 means $ n = 3 $, group 17 means 7 valence electrons ($ 17 - 10 = 7 $).
2. The element in period 3, group 17 is chlorine (Cl). Its electron configuration is $ [Ne]3s^{2}3p^{5} $, in period 3 (row 3) and group 17 (column 17).
# Answer:
Chlorine (Cl)

#### Part c
# Brief Explanations:
1. Period 6 means $ n = 6 $, group 2 means 2 valence electrons (group 2: $ ns^{2} $).
2. The element in period 6, group 2 is barium (Ba)? No, wait, period 6, group 2: radium (Ra)? Wait, no, period 6, group 2: the element is barium? Wait, no, period 6, group 2: let's check. Period 1: H, He; period 2: Li - Ne; period 3: Na - Ar; period 4: K - Kr; period 5: Rb - Xe; period 6: Cs - Rn. Group 2: Be, Mg, Ca, Sr, Ba, Ra. So period 6, group 2 is radium (Ra)? Wait, no, barium is period 6? Wait, barium is period 6? No, barium is period 6? Wait, period 1: 1, period 2: 2, period 3: 3, period 4: 4, period 5: 5, period 6: 6. So group 2, period 6: the element is radium (Ra). Wait, no, barium is period 6? Wait, barium's atomic number is 56, which is in period 6 (since period 5 ends at Xe, atomic number 54; period 6 starts at Cs, 55). So group 2, period 6: radium (Ra)? Wait, no, barium is atomic number 56, which is in period 6, group 2. Wait, yes, barium (Ba) is in period 6, group 2? Wait, no, period 6: Cs (55), Ba (56), La (57) - Lu (71), Hf (72) - Rn (86). So group 2, period 6 is barium (Ba)? Wait, no, radium is atomic number 88, which is in period 7? Wait, I made a mistake. Period 6: elements from atomic number 55 (Cs) to 86 (Rn). Group 2: elements are Be (4), Mg (12), Ca (20), Sr (38), Ba (56), Ra (88). So Ba is atomic number 56, which is in period 6 (since period 5 ends at Xe, 54). So period 6, group 2 is barium (Ba). Wait, but radium is 88, which is period 7. So the correct element is barium (Ba)? Wait, no, let's check the periodic table. Period 1: 1 - 2, period 2: 3 - 10, period 3: 11 - 18, period 4: 19 - 36, period 5: 37 - 54, period 6: 55 - 86, period 7: 87 - 118. So group 2: Be (4, period 2), Mg (12, period 3), Ca (20, period 4), Sr (38, period 5), Ba (56, period 6), Ra (88, period 7). So period 6, group 2 is barium (Ba).
# Answer:
Barium (Ba) (Note: If considering the actinide series, but group 2 is main - group, so Ba is correct for period 6, group 2)

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