Download Name

Name _______________________________________
Entry _________
CHAPTER 4
ATOMIC STRUCTURE AND THE PERIODIC TABLE
PHYSICAL SCIENCE
I. Atomic Structure
A. Objectives
1. Explain _________________________ and describes why it was more
successful than _________________________________________
2. State the ______________________ of each part of an atom according
to the ___________________________________________________
3. Compare and contrast __________________________________ of the
atom
B. What are atoms?
1. Our understanding of atoms required many centuries
a. The idea of an atom – which means _____________________ –
dates back to the Greek philosopher _____________, who lived in
the fourth century BCE.
2. John Dalton developed the ___________________________________
a. Like Democritus, Dalton proposed that ___________________
___________. Dalton’s was the first atomic theory with a
___________________________________
3. An atom is the _____________________________________________
_________________________________________
4. Atoms are the _____________________________________________
C. What’s in an atom?
1. Atoms are made of _________________________________________
a. At the center of each atom is a __________________________
______________________________________________________
b. The nucleus is made of _______ (a subatomic particle that has a
positive charge) and ___________ (a subatomic particle that has
no charge)
c. Moving around outside the nucleus is a ___________________
_____________________________________________________
2. Unreacted atoms have no ____________________________________
a. Although atoms are made of charged particles, they do not have
an overall charge _______________________________________
_____________________________________________________
b. A helium atom is made of _____________________________
_____________________________________________________
D. Models of the Atom
1. Bohr’s model compares electrons to __________________________
a. In 1913, the Danish scientist Niels Bohr suggested that
_________________________________________________ much
like the planets orbit the sun in our solar system
2.
3.
4.
5.
6.
b. In Bohr’s model, electrons can only be in _________________
Electrons act more like _____________________
a. By 1925, Bohr’s model of the atom no longer explained
___________________________________
b. A new model was proposed, in which ____________________
_____________________________________________________
An electron’s exact location __________________________________
a. It is impossible to determine ____________________________
______________________________________________________
b. The best scientists can do is calculate the _______ of finding an
electron in a ___________________________________________
Electrons exist in energy levels
a. The number of filled energy levels an atom has depends on the
____________________________________________________
Electrons are found in ______________________________________
a. An orbital is a _______________________________________
_____________________________________________________
b. An s orbital is shaped like a ______________________
c. A p orbital is __________________ and can be oriented ______
different ways in space
Every atom has between _______________________ valence electrons
a. Valence electrons are found in the ______________ of an atom
and determine the atom’s ________________________________
b. Valence electrons are the ______________________________
_____________________________________________________
II. Section 2: A Guided Tour of the Periodic Table
A. Objectives
1. Relate the organization of the ________________________________
___________________________________________________________
2. Explain why ______________________________________________
3. Determine how many _______________________________________,
given its symbol, _____________________________________________
4. Describe how the __________________________________________
___________________________________________________________
B. Organization of the Periodic Table
1. The periodic table groups similar elements _____________________
a. this organization makes it easier to ______________________
_____________________________________________________
b. elements are listed in order of ________________, because the
periodic law states that when elements are arranged this way,
_____________________________________________________
2. The periodic table helps determine ____________________________
a. horizontal rows in the periodic table are called _____________
b. just as the number of protons an atom has ___________ as you
move from __________________________, so does its number of
_______________________________
3. elements in the same group have ______________________________
a. a group is a _________________________ in the periodic table
b. atoms of elements in the same group have the same number of
_____________________________________________________
4. Some atoms form ___________________
a. an ion is an _________________________________________
_____________________________________________________
b. a lithium atom loses one electron to form a ________________
c. a fluorine atom gains one electron to form a _______________
C. How do the structures of atoms differ?
1. The atomic number, Z, of an atom equals the ____________________
___________________________________________________________
2. the Mass number, A, of an atom equals the ______________________
___________________________________________________________
3. An isotope is an atom that has the ______________________ as other
atoms of the same element do but that has a _______________________
a. example, hydrogen has three isotopes
b. some isotopes are more common than others
4. If you know the atomic number and mass number of an atom, you can
calculate the number of neutrons it has
a. Example: uranium-235 has a mass number of 235. Like all
uranium atoms, it has an atomic number of 92. The number of
neutrons it has is therefore:
Mass number (A):
Atomic number (Z):
Number of Neutrons:
5. Because the mass of a single atom is so tiny, ___________________
__________________________________________________________
6. An atomic mass unit (amu) is equal to _________________________
__________________________________________________________
7. The average atomic mass for an element is a ____________________
__________________________________________________________
III. Section 3: Families of Elements
A. Objectives
1. Locate ______________________________________________ in the
periodic table
2. Locate ___________________________________ in the periodic table
3. Relate an element’s chemical properties to the ____________________
____________________________________________________________
B. How are elements classified?
1. The elements are classified into _______________________________
a. Most elements are metals, ______________________________
_____________________________________________________
b. Nonmetals, all except hydrogen of which are found on the right
side of the periodic table, _________________________________
______________________________________________________
c. Between these groupings are _____________, elements that can
_____________________________________________________
2. The periodic table shows the ______________ of metal, nonmetals and
semiconductors
C. Metals
1. The alkali metals, found in ___________ of the periodic table, are very
______________________
2. The ________________, which include calcium, are found in Group 2
of the periodic table, and are somewhat __________ than the alkali metals
3. The transition metals, __________________________, occupy Groups
3-12 of the periodic table
D. Nonmetals
1. Carbon is found in ________________________ and can form many
compounds
2. Nonmetals and their compounds are ___________________________
3. _______ such as chlorine, are located in ________ of the periodic table
4. _____________, such as neon, make up Group 18 of the periodic table.
They are ___________________________
5. Semiconductors are _________________________________________
6. _________________ is the most familiar semiconductor
a. Silicon is an important part of computer chips, as well as other
semiconductor devices such as __________________________
___________________________________________________
IV. Section 4: Using Moles to Count Atoms
A. Objectives
1. Explain the relationship between a _____________________________
____________________________________
2. Find the molar mass of an element by ___________________________
3. Solve problems converting the ____________________________ to its
____________________________________________________________
B. Counting Things
1. There are many different counting __________: for example, eggs are
packaged by the dozen
2. The mole is useful for _______________________________________
a. a mole (abbreviation: mol) is the ________________________
______________________________________________________
b. Avogadro’s constant is the __________________________ of a
substance (6.022 x 1023)
3. Moles and grams are ______________________
4. The mass in grams of 1 mol of a substance is called its _____________
a. For example, 1 mol of carbon-12 atoms has a molar mass of
12.00 g
b. The molar mass of an element is its ________________, which
is listed in the periodic table.
C. Counting with Moles
1. To convert between _________________ and vice versa, you can use a
conversion factor: ____________________________________________
__________________________
a. Let’s say that a shopkeeper knows that exactly 10 gumballs
have a total mass of 21.4 g. This relationship can be written as
either one of two equivalent conversion factors.
b. What is the mass of exactly 50 gumballs?
i. List the given and unknown values
ii. Write down the conversion factor that converts number
of gumballs to mass.
iii. Multiply the number of gumballs by this conversion
factor, and solve
D. Calculating with Moles
1. An element’s molar mass can be used as a ______________________
2. The diagram below show how to set up the conversion factor,
depending on whether you want to convert from amount to mass or the
other way around
3. Converting amount to mass: Determine the mass in grams of 5.50 mol
of iron.
i. List the given and unknown values
ii. Write down the conversion factor that converts moles to grams.
iii. Multiply the amount of iron by this conversion factor and
solve.
4. Converting mass to amount: Determine the amount of iron present in
352 g of iron.
i. List the given and unknown values
ii. Write down the conversion factor that converts grams to moles
iii. Multiply the mass of iron by this conversion factor and solve