Download Chemical Periodicity

Chemical Periodicity
References:
1 
 CK-12.org – Periodic Table 2 
 Crash Course Chemistry – The Periodic Table This unit begins by reviewing concepts covered in
grades nine and ten science. 1 List the properties of:
metals High density, strong, malleable, and good conductor of heat.
nonmetals Low density, weak, brittle (non-malleable), poor conductor of heat.
metalloids or semimetals High density, in between strong and weak, brittle, fair conductors of heat.
2 Who is Dmitri Mendeleev, and what was his contribution to chemistry? He was a chemist who worked on trying to figure out the periodicity of the periodic table of the
elements. He discovered the arrangement of all the elements.
3 How is the modern periodic table different from the first periodic table? The first periodic table was in columns, not rows, only shows their atomic number.
4 What is the modern periodic law? Characteristics of the elements occur periodically when organized by atomic number.
5 Organization of the periodic table. Indicate where the following are located on the periodic table. 1 periods ：Horizontal rows on the Periodic Table.
2 groups : Numbered column on the Periodic Table.
3 Alkali metals : Group 1 on the Periodic Table.
4 Alkaline Earth Metals :Group 2
5 Halogens : Group 17
6 Noble Gases: Group 18 7 Representative or Main Group elements The S and P on he Periodic table
6. Indicate which elements on the periodic table are:
1 gases at room temperature. Rn, Xe, Kr, Ar, Ne, Cl, F, O, N
1 liquids at room temperature. Br, Hg
h. Transition Metals
Group 3 to group 12
i. Inner Transition Metals
The group of 26 elements on the bottom of the Periodic Table.
k. Lanthanides
: The top row of the Inner Transition Metals.
l. Actinides
: The bottom row of the Inner Transition Metals.
m. metals
: The group of elements from Group 3 to Group 12, plus Aluminum, Gallium, Indium, Tin, Thallium,
Lead, and Bismuth.
n. nonmetals
: Carbon, Nitrogen, Oxygen, Phosphorus, Sulphur, and Selenium.
o. metalloids: Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium.
7. Trends in the periodic table.
electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character.
2 How does the size of the atom vary as you move left to right across the periodic table? Why? The size decreases. This is because the number of electrons decreases as we move in this direction as
well as the nuclear charge.
3 How does the size of the atom vary as you move down the periodic table? Why? The size increases.
This is because the number of electrons increases as we move in this direction as well as the nuclear
charge.
4 What is ionization energy? the amount of energy required to remove the most loosely bound electron, the valence electron, of an
isolated gaseous atom to form a cation.
5 How does the ionization energy vary as you move left to right across the periodic table? Why? It increases, because it is more difficult to remove an electron when the radius of the atom is smaller.
6 How does the ionization energy vary as you move down the periodic table? Why? It decreases, because as the radius grows in size, it becomes easier to remove an electron that is farther
away from the nucleus.
7 What is electron affinity? The amount of chance that a neutral atom will gain an electron.
8 How does electron affinity vary as you move left to right across the periodic table? Why? 9 How does electron affinity vary as you move down the periodic table? Why? It decreases because the electrons are located farther away from the nucleus, making it easier to pull.
10 What is electronegativity? The likelihood of an atom to find electrons to bond with.
11 How does electronegativity vary as you move left to right across the periodic table? It increases there are more positively charged protons in the nucleus which will attract more neutrons.
12 How does electronegativity vary as you move down the periodic table? It decreases, there are less positively charged protons to attract with the neutrons.