Unit 3 Periodic Table Flashcards
Left side of the periodic table:
metals
malleable, ductile
metals
good conductors of electricity
metals
most are solid at room temperature (except for mercury)
metals
right side of periodic table (and hydrogen)
nonmetals
brittle
nonmetals
most are gas at room temperature
nonmetals
located along stair step of periodic table
metalloids
semiconductors
metalloids
Periods
horizontal rows on the periodic table
Groups
vertical columns on the periodic table (also called families)
what groups are transition metals
groups 3-12 or B groups
transition metals are _____ luster
high
inner transition metals
lanthanides: bellow periodic table (first row)
actinides: bellow periodic table (second row)
Halogens
Group 17
-most reactive nonmetals
Nobel Gases
group 18
-Stable atoms that don’t bond with other elements (inert)
-nonflammable and nonreactive
Alkali metals
first group of periodic tables
-most reactive metals
where are Alkaline Earth metals
group 2 in periodic table
Electron Cloud
area round nucleus where electrons are likely to be found.
Orbitals
3d regions around the nucleus that describe probable locations of electrons
What are the four types of sublevels?
s, p, d, f
how many orbitals dose each sublevel have?
s=1
p=3
d=5
f=7
How many electrons can each sublevel hold?
s=2
p=6
d=10
f=14
each orbital can hold ___ electrons?
2
Electron Configuration
the arrangement of electrons in an atom
An electron occupies the ________ energy orbital that can receive it.
lowest
2 electrons that occupy the same orbital must have ______ ___________.
opposite spins
How do orbitals of the same energy fill up?
each orbital is occupied by 1 electron before any orbital is occupied by a 2nd electron.
In the Sublevel 3s^2 what dose “3” represent
3 represents the energy level.
Valence Electrons
the electrons in the outermost energy level (energy shell)
Oxidation number
the charge of an ion
stable
an atom with a full outer energy shell
period number =
the number of energy levels
for non-transition elements, group number=
number of valence electrons
For transition metals, the number of valence electrons is:
all electrons in the highest value of n (energy level), and unfilled d or f shells
Octet rule-
chemical compounds form so that each atom has a full set of electrons in its highest energy level.
Trend in atomic radius and atomic character across the periodic table:
increases as you go down the periodic table
decreases as you go from left to right
Trend in electronegativity and ionization energy across the periodic table:
decreases as you go down the periodic table
increases as you go from left to right
Cation
a positive ion
-metals from cations
Anion
a negative ion
-nonmetals from anions
Ionization energy (IE)
energy needed to remove an electron from a neutral ion
-the greater the number the harder it is to remove an electron
Each successive electron removed requires ________ energy.
more
electronegativity
the ability of an atom to attract electrons.
metalic character
ser of chemical properties associated with metal on the periodic table.
-ability to lose electrons (easily achieve octet)
-low ionization energy
-low electronegativity
Most metallic elements
bottom left
What elements along the stair of the periodic table are not Metalloids?
Aluminum (Al), Astatine (At)
