Introduction to Periodic
The periodic table is arranged in the order of ...
These type of elements have low first ionization energy and electronegativity.
Metals
At STP, this metal is liquid.
Hg (mercury)
This element has the smallest atomic radius on the periodic table.
He (Helium)
In which area of the Periodic Table are the elements with the strongest metallic properties located?
Lower left
Who discovered the modern day periodic table?
Henry Mosely
This group of elements is best described as being lack luster and brittle...
Nonmetals
This group consists of the most reactive metals on the periodic table.
Group 1 (Alkali Metals)
In terms of the shielding effect, explain why the atomic radius increases as you move down a group.
As you move down a group on the periodic table, the atomic radius increases because the shielding effect becomes more pronounced, meaning that the outer electrons experience less attraction from the nucleus due to the increasing number of inner electron shells acting as a barrier, effectively pushing the outermost electrons further away from the nucleus and enlarging the atomic radius.
Which element has the highest boiling point?
a. Boron
b. Nitrogen
c. Sodium
d. Silicon
a. Boron
How do periods and families differ?
Periods = horizontal (run left to right)
Families = vertical (run up and down)
Explain why silver is a good conductor of an electricity in terms of electrons.
Silver is a metal that can conduct heat and electricity due to its “sea of mobile electrons.”
They both contain 5 valence electrons.
Define electronegativity and identify its trend of increase on the periodic table.
Electronegativity is the attraction for electrons. The larger the electronegativity, the more an atom attracts electrons.
Electronegativity increases as you go from left to right and decreases as you down the group.
Which element has the lowest density?
a. Lithium
b. Neon
c. Niobium
d. Radon
b. Neon
What do all the atoms in the same period have in common?
The same number of Principle Energy Levels (PELs) or shells.
Based on Table J, which metal is more active than calcium, but less active than cesium?
a. Potassium
b. Lithium
c. Iron
d. Barium
d. Barium
Identify the group of the periodic table that is inert (not reactive) and explain why it is inert.
Noble Gases (Group 18)
They are inert because they have a stable electron configuration (8 valence electrons) aka a full octet.
What is a diatomic element?
Identify the 7 diatomic elements.
Extra 100: Identify the group on the periodic table that mainly contains these type of elements!
Diatomic element: An element that is unstable alone in nature. Therefore, it pairs up with a second atom of itself to share valence electrons to fill their valence shells.
HOFBrINCl: Hydrogen, oxygen, fluorine, bromine, iodine, nitrogen, & chlorine
Ex: H2, O2, F2, Br2, I2, N2, Cl2
Extra: Group 17 (Halogens)
As you move down a group on the periodic table, what is added?
A Principle Energy Level (PEL) or electron shell.
Describe the physical properties of metalloids and list 6 of the metalloids on the periodic table.
Metalloids have both metal and nonmetal properties.
Metalloids: Boron, Silicon, Germanium, Arsenic, Antimony, and Tellurium
This group contains elements of all three phases of matter at STP.
Group 17 (Halogens)
Why does Rb have a low first ionization energy as opposed to Cl?
Explain using the following terms: Valence electrons, energy, and octet.
Rb is a metal which has 1 valence electron. It easily loses its electron which will allow it to achieve an octet. Therefore has a lower amount of energy to do this.
Cl has 7 valence electrons and only needs one more to achieve an octet. Therefore, it does not want to lose an electron as easily, and it takes more energy for Cl to lose an electron than for Rb.
At STP, graphite and diamond are two solid forms of carbon. Explain why these two forms of carbon have different physical properties.
These are allotropes of carbon therefore they have different molecular/crystal structures.