Download Chapter 4 Structure of Atoms Isotopes and Ions KEY

KEY Chapter 4-2 Review Atoms, Isotopes and Ions
Complete the diagram of an atom below with these terms; nucleus, proton, neutron, electron, 1st energy level, 2nd
energy level. The electrons are located in the _electron cloud_ _ .
neutron
1st energy level
proton
nucleus
2nd energy level
particle
proton
neutron
Electron
Symbol
P+
n
e-
electron
Properties of Subatomic Particles (pg 109)
Relative charge
Relative mass (atomic mass units or amu)
+1
1
0
1
-1
0
Definitions
Atomic mass- average mass of all the isotpes of an element
Atomic number- number of protons in the nucleus
Mass number- neutrons + protons in the nucleus
Atom- smallest particle of an element
Isotope- atoms of a given element that have different numbers of neutrons and different mass numbers.
Ion- an atom or isotope that has positive or negative charge
Questions
1. List the charge and location of protons, neutrons and electrons in an atom.
protons positive one, Nucleus
Elecrons- negative one, -1, in electron cloud
neutrons no charge, nucleus
2. List the relative mass of protons, neutrons and electrons in an atom. Relative mass means the mass compared to
the other particles.
Protons, neutrons 1 atomic mass unit (amu),
electrons have a mass of 0 amu
3. Label this “symbol square” with these words; net charge, mass number, and atomic number, symbol of ele
Mass number
Atomic number
Or
number of
protons
Net Charge
Symbol of element H - hydrogen
How many electrons fit in each energy level?
first – 2 maximum
second – 8 maximum
third - 18 maximum
5. Describe how to calculate the number of protons and neutrons in an atom using the atomic number and the mass
number.
Protons = atomic number
Neutrons: mass number – atomic number (larger number – smaller number in “symbol square”)
6. Describe how to calculate the number of electrons from the net (overall) charge.
Protons – electrons = net charge
7. Describe the similarity between each atom and its isotope.
Same # OF PROTONS, But
different # of neutrons & different mass numbers
8. What pattern do you see with the subatomic particles (protons, neutrons, and electrons) in each of the ions that
you created?
Protons
≠ electrons
Protons & neutrons unchanged
Neutral Atom (stable form)
Isotope (stable form)
Ion (stable form)
KEY Neutral Atom (stable form)
2) name _____________ p+ = 2
3) name _____________
n= 1
p+ = _____
Isotope (stable form)
e- 2
n= _____
e - ______
Ion (stable form)
none
none
p+ = ____
n = _____
e - _____
p+ = ____
n = _____
e - _____
7
4) name _____________
p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
Unstable
p+ = ____
n = _____
e - _____
5) name _____________
p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
p+ = ____
n = _____
e - _____
11
6) name _____________ p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
p+ = ____
n = _____
e - _____
-4
7) name ____________
p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
p+ = ____
n= 7
e - 10
-3
8) name _____________ p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
17
p+ = ____
n = _____
e - _____
16
-2
16
9) name _____________ p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
p+ = ____
n = _____
e - _____
NONE
10) name ___________ p+ = _____
n= _____
e - ______
p+ = ____
n = _____
e - _____
p+ = ____
n = _____
e - _____
Describe the pattern in the way that the electrons are organized on the atoms. You may use your textbook for help.
First energy level filled w/2 electrons; second energy level filled with 8 electrons
What pattern do you see with the subatomic particles (protons, neutrons, and electrons) in each of the neutral atoms
that you created?
Protons = electrons
Protons + neutrons = mass number