unit 5 section 2 notes a guided tour of the periodic table
TRANSCRIPT
Unit 5 Section 2 Unit 5 Section 2 NotesNotes
A Guided Tour of the Periodic A Guided Tour of the Periodic TableTable
Who is Dmitri Mendeleev? Who is Dmitri Mendeleev? (1834-1907)(1834-1907) In 1869, Dmitri Ivanovitch Mendeléev
created the first accepted version of the periodic table.
What is the Periodic Table?What is the Periodic Table? Shows all known elements in the universe Organizes elements by chemical
properties
The Periodic TableThe Periodic Table The periodic table groups similar elements
together. This organization makes it easier to predict the properties of an element based on where it is in the periodic table.
ElementsElements Elements in the periodic table are
represented by their symbols. The first letter is ALWAYS capital If there is a second letter, it is ALWAYS
lowercase Every element has its own unique symbol
CCarbon
Cu
Copper
How is the Periodic Table How is the Periodic Table Organized?Organized? The elements are arranged based on the
number of protons in the nucleus. Periodic Law: states that when elements
are arranged in order of increasing atomic number, similarities in their properties will occur in a regular pattern.
Periods in the Periodic Periods in the Periodic TableTable Period: a horizontal row of elements in the
periodic table As you move from left to right in a period, the
number of protons and electrons increases by one Elements in the same period DO NOT have similar
properties; in fact, they change greatly across the row
The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.
Groups or Families in the Groups or Families in the Periodic TablePeriodic Table Group or family: a vertical column of
elements in the periodic table All elements in a family have the same
number of valence electrons, so they have similar properties For example, lithium (Li), sodium (Na),
potassium (K), and other members of group 1 are all soft, white, shiny metals.
These elements are NOT exactly alike because they have different numbers of protons
IonsIons Ionization: the process of adding electrons
to or removing electrons from an atom Ion: an atom that has lost or gained one or
more electrons and has a net electric charge
Cation: an ion with a positive charge Anion: an ion with a negative charge
Goal of Atoms All atoms want to have a FULL octet (8 e-
in outer shell) They do this by gaining, losing, or sharing
electrons
Metals and Electrons Metals LOSE electrons to form cations Example: Lithium loses one electron to
become a lithium ion, written as Li+
3 p+
4 n0
Second energy level can hold up to 8 e-. It is easier to lose 1 e- than gain 7 more.
3 p+
4 n0
3 electrons2 electrons
After lithium loses an electron, it has a full outermost energy level.
Nonmetals and Electrons Nonmetals GAIN electrons to form anions Example: Fluorine gains one electron to
become a fluoride ion, written as F-
9 p+
10 n0
9 p+
10 n0
9 electrons 10 electrons
Second energy level can hold up to 8 e-. It is easier to gain 1 e- than lose 7 more.
After fluorine gains an electron, it has a full outermost energy level.
Atomic NumberAtomic Number Atomic Number: how many protons are in
the nucleus of an atom Remember that ATOMS are neutral, so
they have equal numbers of protons and electrons Therefore, atomic number also tells the
number of electrons for atoms only
Mass Number (Atomic Mass Number (Atomic Mass)Mass) Mass Number: the number of protons and
neutrons in an atom Mass number is ONLY protons and neutrons
because they provide most of an atoms mass The same element can have different
mass numbers because they may have different numbers of neutrons.
IsotopesIsotopes Isotopes: atoms of the same element
having the same number of protons but different numbers of neutrons Each “version” of the atom has the same
number of protons and electrons
Calculating Neutrons in an Calculating Neutrons in an atomatom To calculate the number of neutrons in an
atom, take mass number minus atomic number.
Mass Number
- Atomic Number
# of Neutrons
Average Atomic MassAverage Atomic Mass In the periodic table, the atomic mass is a
decimal because it is an average of all the naturally occurring isotopes
When calculating neutrons from average atomic mass, round to the nearest whole number
Example: How many neutrons are in Zinc? (Atomic Number 30; Average atomic mass 65.39) 65-30 = 35 neutrons