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PT History
PT Arrangement
Group Properties
Trends Definitions & Patterns
Element Trends
100
Dmitri Mendeleev
Who was the inventor of the first periodic table?
100
Location of the alkali and alkaline earth metals
What are groups 1A and 2A?
100
This family is stable and unreactive. Explain why.
What are the noble gases, they have a full outer shell and do not want any more electrons.
100
This term means 1/2 the distance between to adjacent nuclei.
What is atomic radius?
100
Larger atomic radius Na or Ba; Rb or Br?
What is Ba; Rb?
200
increasing atomic mass
What is the way in which Mendeleev arranged the periodic table?
200
Describe where metals, nonmetals, and metalloids are located.
What is to the left of the stair step (metals) to the right of the stair step (non metals) and bordering the stairstep (metalloids)?
200
Halogens react readily with____________to form salts.
What are the alkali metals?
200
Define electronegativity.
What is an atom's ability to attract electrons to itself when bonding to other atoms.
200
Larger Ionization energy Li or S? N or Sb?
What is S and N?
300
Who rearranged the periodic table and how?
Who was Henry Mosley Increasing Atomic Number
300
Location of the Halogens and Noble gases?
What is 7A (halogens) & 8A (noble gases)?
300
These metals are the most reactive. Explain why.
What is alkali metals, they have only one valence electron to give up and do so willingly.
300
Define Ionization Energy.
What is an atoms ability to hang onto it's valence electrons?
300
Larger electronegativity Mg or O; Ca or Ba
What is O and Ca?
400
What are the representative elements, and what does that mean?
1A-8A, they represent a wide variety of chemical and physical properties of all elements.
400
Location of the transition & inner transition metals and name the 2 periods of the inner transition metals.
What are groups 3-12 and the out block? What are lanthanides and actinides?
400
Hydrogen can be considered a member of these 2 groups, and explain why.
What is Alkali metals and halogens, because it has 1 valence electron, it acts like both groups.
400
Trend for atomic radius across periods and down groups, and why?
What is decreasing across periods because there are more protons to pull the levels closer to the nucleus, and increasing down a group because there are more levels literally making the atom larger?
400
Which is larger, S or it's ion and why?
What is Sulfurs Ion. It has gained two electrons making it larger?
500
Define periodic law.
What is elements arranged in order of increasing atomic number, there is a repetition of their physical and chemical properties.
500
This group's electron configuration ends in d7
What is group 7 (transition metals)?
500
Most reactive metal and nonmetal, why?
What is Francium (metal) Fluorine (nonmetal). Francium only needs to give up one valence electron, and with all of it's electron orbitals, it is a distance from the nucleus, so there isn't a strong hold on it. For Fluorine, it only needs one valence electron, and has only 2 orbitals, so it has a strong attraction for them.
500
Trend for Ionization energy and electronegativity across a period and down a group and why?
What is IE: increasing across a period because the number of protons increases, creating a stronger hold on the atoms valence electrons; decreasing down a group because the levels increase causing a decreased hold on the valence electrons? Electronegativity: increases across a period because there is an increased number of protons in the nucleus causing an increased attraction to other electrons; decreases down a group because there are more levels, putting the nucleus farther away from electrons it could attract.
500
Larger Electronegativity: Ca or Cs; Si or S and why?
What is Ca (less energy levels) and S (more protons)