Periodic Table & Periodic Trends Unit Test Study Guide
Name the three classes of elements
metals, nonmetals, metalloids
As you move from left to right across a period, the first ionization energies _____
increase
Do metals tend to have high or low electronegativities?
low
m or nm : are not conductors
nm
m or nm : dull, brittle
nm
m or nm : gain electrons
nm
The horizontal rows of the periodic table are called _____
periods
What is the best reason that the atomic radius generally increases moving down a group of elements.
the number of occupied energy levels increases
What has more ionization energy? Al vs S
S
This scientist predicted that the empty spaces on his periodic table represented _____
Undiscovered elements
The number of valence electrons are in group 17 elements is _____
7
This group's name means "basic".
Alkaline Earth Metals (Group 2)
List in order of smallest to largest: Cu, Cu-, Cu+
Cu+, Cu, Cu-
Who is attributed with the idea of arranging the known elements of his time in a table according to their chemical and physical properties?
Dmitri Mendeleev
Which atom or ion will have the larger radius: F or F-
F-
Which of the following atoms is smallest: nitrogen, oxygen, or fluorine?
Fluorine
What element is the most electronegative?
Fluorine (F)
Explain why atomic radius decreases going across the period left to right on the periodic table.
Going across, the positive nuclear charge increases with more protons. This attracts electrons towards the nucleus giving a smaller atomic radius.
What is the trend for reactivity for the halogens group?
Going down, reactivity decreases
What is the trend for reactivity for the alkali metal group?
Going down, reactivity increases
Four groups 13 through 18, the number of valence electrons is equal to ______
Group # -10
This class of elements have both metallic and nonmetallic properties.
Metalloids
What has more ionization energy? N vs Si
N
Which had a higher atomic radius? N vs F
N
This group is unreactive, and only found in pure form in nature.
Noble Gases (group 18)
What is more electronegative? O vs Cl
O
Which of these elements have the highest ionization energy: aluminum, silicon, or phosphorous?
Phosphorous
Which is larger than the neutral atom? S-, S, S+
S-
Which is the largest? S vs S-2
S-2
Which of these elements has the highest ionization energy: tin, arsenic, or sulfur?
Sulfur
What is the general trend of electronegativity as you go down the group on the periodic table?
The electronegativity decreases as you go down the group.
Write a definition for ionization energy.
The energy required to remove an electron.
Period 5, group 14
Tin (Sn)
This group of metals contains group 3-12.
Transition Metals (Group 3-12)
What are valence electrons?
electrons found in the outermost energy level of atoms
The vertical columns of the periodic table are called ______
groups
m or nm : good electrical conductors
m
m or nm : lose electrons
m
m or nm : malleable, ductile
m
These elements are found in the second row of the f-block elements.
Actinides (Group 3)
What has a higher atomic radius? N vs Al
Al
Which of the following is the smallest: a lithium atom, Li+ ion, or a sodium atom?
Li+ ion
This group contains the most reactive group of metals.
Alkali Metals (Group 1)
Period 3, group 17
Chlorine (Cl)
Which atom or ion will have the larger radius: F- or Cl-
Cl-
The most reactive group of nonmetals
Halogens (Group 17)
As you move from the top of a group to the bottom, the first ionization energies _____
decrease
This periodic law states there is a periodic repetition of physical and chemical properties of the elements _______
when they are arranged in order of increasing atomic number
Which atom would it take more energy to remove its first electron: sodium or aluminum?
Aluminum
Which of the following atoms is largest: nitrogen, phosphorus, or arsenic?
Arsenic
Period 6, group 2
Barium (Ba)
Which is the largest? Ca vs Ca+2
Ca
List the following atoms in order of decreasing electronegativity: Cl, K, and Zn.
Cl, Zn, K
Which is the correct order of ionization energy from highest to lowest? Al, Si, Cl, P, S
Cl>S>P>Si>Al
Who arranged the periodic table of elements in the order of atomic number?
Henry Moseley
Definition for electronegativity
How well an element can attract electrons.
Which atom or ion will have the larger radius: K+ or Ca2+
K+
Which atom or ion will have the larger radius: Na+ or K+
K+
Which is smaller than the neutral atom? K-, K, K+
K+
Each period of the periodic table corresponds to ______
principal energy level
Define atomic radius
size/radius of an atom
Define ionic radius
size/radius of an ion
What do elements in the same periodic periods have in common?
the same number of principle energy levels
What do elements in the same periodic group have in common?
the same number of valence electrons
Which of these is the largest atom: phosphorous, sulfur, or chlorine?
Phosphorous
