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Terms in this set (27)
What did Mendeleev do? How did he arrange the elements?
developed 1st periodic table. He arranged the known elements at the time in order of increasing atomic mass.
What did Moseley do? How did he arrange the elements?
reordered ordered the periodic table by atomic numbers rather than by weight, thereby modifying the Periodic Law.
What did Newlands do?
number sequence in order of their atomic weights, beginning with Hydrogen. This showed "The eighth element, starting from a given one, is a kind of repetition of the first
What did Meyer do?
compiled a Periodic Table of 56 elements based on the periodicity of properties such as molar volume.
What did Lavoisier do? how did he arrange the elements?
developed the first extensive element list, of 33, separating metals from non-metals, dividing the few elements known in the 1700's into four classes, and discovering Oxygen and Hydrogen
How is the current periodic table arranged?
By atomic number
What is the periodic law?
when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.
How do some periodic tables show what elements are representative elements?
label them group A
How do some periodic tables show what elements are Transition elements?
label the group B
How do you know the number of valence electrons just from looking at the periodic table?
the group number will tell you
Which groups are the representative elements found in?
groups 1 through 2 and groups 13 through 18
Which groups are the transition metals found in?
groups 3 through 12 in the middle of the periodic table.
what properties do transition metals have?
solid at room temperature (except for Mercury)
Where are the inner transition metals found on the periodic table?
underneath the periodic table. They're called the lanthanide and Actinide series.
What properties do inner transition metals have?
These metals are also solid at room temperature
How many groups and how many periods are on the periodic table?
There are groups and periods in the periodic table.
Where are alkali metals found? How many valence electrons do they have in their outermost energy level? how (un)stable and reactive are they? are they likely to bond? What is their consistency like? how abundant are they in nature? What are some chemical and physical properties (list 3)?
-low densities, and, low melting, and boiling points.
Where are alkaline earth metals found? How many valence electrons? How reactive are they?
-highly, likely to bond and lose 2 electrons
Where are Halogens found? How many valence electrons?
-7 so they'll want to gain 1 more electron to make their outer energy level full
Where are noble gases found? How many valence electrons? How stable? Do they naturally bond with other elements? List 5 properties that they have.
-high densities, high melting points, colorless, odorless, and tasteless
What kind of elements does the Lanthanide series include? Where is the Lanthanide series found on the periodic table?
-"rare Earth elements"
-top row of the inner transition metals, these elements are part of period 6
What kind of metals does the actinide series include? Where can the actinide series be found on the periodic table?
-the bottom row of the inner transition metals, these elements are part of period 7.
Define atomic radius. the atomic radius --- across a period and --- down a group.
the distance from the atom's nucleus to the outer edges of the electron. The atomic radius decreases across a period and increases down a group.
Define ionic radius
the distance from the nucleus to the outer edge of the electron cloud of an ion.
Define ionization energy. --- as you go down a group and --- as you go down a period.
The amount of energy required to remove an electron from an atom. decreases as you go down a group and increases as you go down a period.
What 2 things does ionization energy depend on?
-distance between electron and nucleus (culem law)
-nuclear charge (# of protons)
Define electronegativity. --- as you go down a group and --- as you go across a period.
tendency for an element to attraction electrons when chemically combined w/ another element. increases and increases
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