Name ____________________________________________Period______Date___________________
The Periodic Law - 5-1
___C___1. In the modern periodic table, elements are ordered
(a) according to decreasing atomic mass
(c) according to increasing atomic number
(b) according to Mendeleev’s original design
(d) based on when they were discovered
__ D___2. Mendeleev noticed that properties of elements appeared at regular intervals when the elements were
arranged in order of increasing
(a) density
(b) reactivity
(c) atomic number
(d) atomic mass
__ B___3. The modern periodic law states that
(a) no two electrons with the same spin can be found in the same place in an atom
(b) the physical and chemical properties of the elements are functions of their atomic number
(c) electrons exhibit properties of both particles and waves
(d) the chemical properties of elements can be grouped according to periodicity, but physical properties
cannot
___C___4. The discovery of the noble gases changed Mendeleev’s periodic table by adding a new
(a) period
(b) series
(c)group
(d)sublevel block
___D___5. The most distinctive property of the noble gases is that they are
(a) metallic
(b) radioactive
(c) metalloids
(d) largely unreactive
___C___6. Lithium, the first element in Group 1, has an atomic number of 3. The second element in this group has an
atomic number of
(a) 4
(b)10
(c) 11
(d) 18
7. An isotope of fluorine has a mass number of 19 and an atomic number of 9.
___9__a. How many protons are in this atom?
__10 _b. How many neutrons are in this atom?
c.What is the symbol of this fluorine atom including its mass number and atomic
19
__ 9F__number?
8. Samarium, Sm, is a member of the lanthanide series.
__Plutonium
_ a. Identify the element just below samarium in the periodic table.
_____32 ________ b. The atomic numbers of these two elements differ by how many units?
9. A certain isotope contains 53 protons, 78 neutrons, and 54 electrons.
________53_______ a.
________131______ b.
________I ______ c.
__F, Cl, Br, At ____ d.
What is its atomic number?
What is the mass of this atom in amu’s (to the nearest whole number)?
Is this element Pt, Xe, I, or Bh(107)?
Identify two other elements that are in its group.
10. Identify the element, and write the valence (very last e-) for each of the following:
_______Ge: 4p2_____________a. the Group 14 element in Period 4
_____ Bi: 6p3_____ ________b. the only metal in Group 15
___
Sc: 3d1
_________c. the transition metal with the smallest atomic mass
2
_______Ra: 7s
_________d. the alkaline earth metal with the largest atomic number
11. There are 18 columns in the periodic table; each has a group number. Give the group numbers that make
up each of the following blocks:
__1-2___ a. s block
__13-18__ b. p block
_ 3-12 _ c. d block
12. Using the four elements below-left, answer the following:
a. Which element is more like lithium in terms of properties: Na
b. Which element has a lower melting point: Li
c. Which element is closer to achieving noble gas configuration: Li
d. Which element is a better conductor of electricity: Na
The Periodic Law 5-2
Use only this periodic table to answer the following questions.
13.
On the periodic table above are several areas labeled A—H.
____p____ a. Area A represents which block: s, p, d, or f ?
b. Identify the remaining labeled areas of the table, choosing from the following terms: main-group elements,
transition elements, lanthanides, actinides, alkali metals, alkaline-earth metals, halogens, noble gases.
_____Alkali Metals _____ B
___Halogens
__Alkaline Earth Metals
___Noble Gases
__Transition Metals
__ C
____ D
___Actinides
____ F
_____ G
______ H
__Main Group Elements __ E
14. Using the answers to B, C, D, F, & G above, answer the following:
a. The __________B_________ have a single e- in the highest energy level?
b. The __________C_________ achieve the e- configurations of noble gases by losing two e-.
c. The __________D_________vary in the number of e- in the valence energy level.
d. The __________F_________achieve e- configuration of noble gases by gaining one e-.
e. The __________G_________ have full s & p orbitals in the highest occupied energy level.
f. The __________F_ _______ are highly reactive and readily form salts with metals.
g. The __________G_________ are stable and unreactive.
h. The __________C_________ are metals that are more reactive than the transition elements but less reactive than
the alkali metals.