Elements
Where are Metalloids located on the periodic table?
What is...
On the stair-step line.
What is...
Valence electrons.
List the following elements in order of INCREASING electronegativity
F, Li, C
What is...
Li < C < F
Periods (Rows) on the Periodic Table all have the same number of ________
Energy Levels
Which element is often considered the building block of life?
What is...
Carbon.
What element from the Carbon group is a large component of sand?
What is...
Silicon.
Which periodic trend involves taking an electron AWAY from an atom?
What is...
Ionization energy
On the periodic table, the ionization energy increases in what direction?
(i.e. down and right, up and left, up and right, down and left)
What is...
Up and to the right
What kind of elements (metal, metalloid, nonmetal) are NOT shiny, are various colors, and are poor conductors of electricity?
What is...
Nonmetals
What element is the largest component of the air that we breathe?
What is...
Nitrogen
Which elements are diatomic?
(Name all 7)
What are...
Hydrogen, Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, and Iodine
Which periodic trend involves...the ability to attract electrons in a chemical bond?
What is...
electronegativity.
List the following elements in order of SMALLEST to largest ATOMIC RADIUS:
Ni, F, Ba
What is...
F < Ni < Ba
What is the name for the 7th group (column) of elements?
What is...
Halogens.
Which Halogen is used by the thyroid and is important for metabolism?
What is...
Iodine
In regards to Coulomb's Law,
How does the distance between charges impact the attractive force between the two particles?
As the distance increases, the attractive force decreases.
How does the number of protons in the nucleus impact the Coulombic Attraction (attractive force) within the atom (within a row on the periodic table)?
What is...
Causes the attractive force to increase (which will result in the atomic radius shrinking)
Which of the following IONS has a larger atomic radius?
O-2 OR N-3
What is...
N-3
What is the effective nuclear charge?
The "net" effect of the positive charge of the nucleus of an atom on the valence electrons.
Noble Gases do NOT follow which of the 3 periodic trends that we covered in class?
What is...
Electronegativity
We talked about how ionization energy is related to the conductivity of a substance.
In the context of ionization energy and how tightly electrons are held, why are non-metals poor conductors of electricity?
Non-Metals have a high ionization energy which means electrons are held tighter by the element and do not freely move (i.e. are not able to conduct electricity).
Why does Ionization energy increase as you move left to right across a period (row) of the periodic table?
What is...
The effective nuclear charge increases.
Electrons are more strongly attracted to the nucleus.
They are harder to pull off the atom.
Why are cations smaller than their atom?
i.e. why is Al+3 is smaller than Al
What is...
Al+3 loses an energy level when becoming an ion
WHY does a Sulfur atom have a SMALLER atomic radius than a Phosphorus atom?
What is...
A Sulfur atom has more protons in the nucleus. As a result, the electrons in the outer energy level experience a larger effective nuclear charge, drawing them closer towards the nucleus, thus decreasing the radius.
Which of the following has the largest radius of the three atomic/ionic species. Make sure to defend your answer.
O-2 O Na+1
What is...
O-2. The Oxygen atom can be eliminated because anions are always larger than the atom (due to electron repulsions). O-2 and Na+1 are part of an isoelectronic series. They have the same number of electrons but because Na+1 has more protons, the attractive forces are greater, shrinking the radius more.