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Periodic Table of Elements
Chemistry Unit 5 Review
Terms in this set (28)
Who is credited with developing the first periodic table? How did he organize the elements?
Dimitri Mendeleev, by increasing atomic mass
Henry Moseley even improved the periodic table by organizing the elements based on what?
by increasing atomic number
If you know the location of an element on the periodic table, you can predict its...
The elements in the same period of the periodic table have the same number of
The elements in the same group of the periodic table have the same number of
Why are noble gases relatively unreactive?
because they have a full outer energy level
Identify, by number, the groups located within the s-block, within the p-block, and within the d-block
What is the name of Group 1? What are 2 characteristics of elements within that group?
Alkali Metals, Only 1 valence electron, extremely reactive
What is the name of Group 2? How does the properties of the elements within this group compare with those of the alkali metals?
Alkaline Earth Metals, has 2 valence electrons, is reactive but not as much
What is the mane used to refer to the entire set of d-block elements?
Which group is called the halogens?
What are metalloids? And where are they on the periodic table?
Have properties of metals and nonmetals, on the stair-step line
What is an atomic radius?
the distance from nucleus of one atom to the outer electron of another
What trend is observed among the atomic radii of main group elements across a period? And down a group?
Decreases across, increases down
An atom with a positive charge
An atom with a negative charge
What is Ionization Energy?
Energy required to remove an electron from a neutral atom to form a positive ion
How does the first ionization energies of main group elements vary across a period and down a group? Explain Why
Increases across because each next element increases protons, Decreases down because of the number of energy levels (distance)
How does the size of a cation compare to the size of the neutral atom from which it is formed? How does the size of an anion compare?
Cation smaller, Anion bigger
What are valence electrons?
The electrons in the outermost energy level
What is electronegativity?
The ability of an atom to attract electrons from another atom in the compound
The most electronegative element
The least electronegative
Most reactive metals are found in Group?
Most reactive nonmetals are found in Group?
Why do halogens readily form (-1) ions?
Because they have 7 valence electrons and they want 8
What is the trend in electronegativity going down a group?
What is the trend in electronegativity across a period?
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