Download A Periodic Table Logic Problem

Name: _____________________________ Block: _______________ Date:_______________
A Periodic Table Logic Problem
Objectives: To analyze the properties and relationships of 26 elements
Identify each element’s place in the periodic table based on these properties
and relationships.
Introduction: When elements are arranged in the periodic table in order of increasing atomic
number, there is a periodic repetition of their physical and chemical properties. The way
properties change from left to right across a period and from top to bottom within a group are
called periodic trends. Here is a summary of some periodic trends.
Atomic size can be expressed by a measurement call the atomic radius. Atomic radius is
one half the distance between the nuclei of two atoms of the same element when the atoms are
joined. The atomic radius generally increases from top to bottom within a group. The atomic
radius generally decreases from left to right across a period.
Ionization energy is the energy required to remove and electron from an atom. This
energy is measured when the atom is in the gaseous state. The first ionization energy is the
energy required to remove the first electron from an atom. The second ionization energy is the
energy required to remove an electron from a cation with a 1+ charge. The third ionization
energy is the energy required to remove an electron from a cation with a 2+ charge. The second
ionization energy is always larger than the first ionization energy. The third ionization energy for
an element is always larger than the second ionization energy. In general, the first ionization
energy decreases from top to bottom within a group and increases from left to right across a
period.
Electronegativity is the ability of an atom of an element to attract electrons when the atom
is in a compound. In general, electronegativity values decrease from top to bottom within a
group and increase from left to right across a period. Because noble gases do not tend to form
compounds, electronegativity values for noble elements are usually omitted from data tables.
Metals tend to have low first ionization energies and low electronegativity values.
Nonmetals tend to have high first ionization energies and high electronegativity values.
Purpose: In this experiment, you will use a series of clues to arrange a set of unknown
elements in a periodic table. The elements are the elements with atomic numbers 1-20 and 3136. A letter of the alphabet is used to represent each unknown element. The letter designation
is not related to an element’s chemical symbol. Each clue refers to a property of an element or a
relationship an element has to other elements in the periodic table. Along with logic and
knowledge of properties, you will use periodic trends to solve the puzzle. When you are done,
each element will be in its unique place on the table. Good luck!
1A
2A
3A
4A
5A
6A
7A
8A
Name: _____________________________ Block: _______________ Date:_______________
Directions: Using the clues below, place the letter of each element in its place on the periodic
table given to you.
A Has one of the highest electronegativities on the table
B Has one electron in a 3p orbital
C Has five electrons in the fourth energy level
D Forms the smallest 2+ ion
E Tends to gain one electron
F Electronic configuration is 1s22s22p63s23p3
G Is the most electronegative element
H An ion of this element with a 2+ charge has 18 electrons
I Its second ionization energy is large compared to its first ionization energy
J Its highest occupied energy level is full
K This nonmetal is likely to form an ion with a 3- charge
L Has the highest first ionization energy in the table
M Has the smallest atomic radius in the third period
N Is the smallest atom in its group
O The first element with an electron in the second energy level
P The only nonmetal in a group with highly reactive metals
Q Has eight fewer protons than its “groupmate” H
R The most likely element of the ones included to lose an electron
S A metalloid in period 4
T Its ionic radius is larger than its atomic radius
U The ion with a 2- charge that it forms has 18 electrons
V Atomic number is 34
W Metalloid that forms an ion with a 3+ charge
X Has characteristics of both a metal and a nonmetal
Y Has a lower first ionization energy than S
Z Has a first ionization energy that is higher than T but lower than M