Download NAME DATE PER EKS 2: Atomic Structure Quiz Study Guide Level 2

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DATE
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EKS 2: Atomic Structure Quiz Study Guide
Level 2 Vocabulary
Atom: smallest unit of matter. Looks like planetary model, with a dense positively charged nucleus in the
middle, and electrons orbiting the outside.
Isotope: heavier and lighter versions of the same element. The masses of isotopes differ because they
have different amounts of neutrons.
Ion: an atom with a net electrical charge. Ions have charges because they gain or lose electrons.
Negatively charged ions (anions) gain electrons. Positively charged (cations) ions lose electrons.
Proton: positively charged particle located in the nucleus. The number of protons defines the atom and
never changes.
Neutron: neutral particles located in the nucleus.
Electron: negatively charged particles that make up most of an atom’s volume.
Atomic Number: small number on the periodic table, number of protons an element has
Mass Number: how heavy an atom is, can be calculated by adding P+N
Chemical Symbol: 1 or 2 letter abbreviation for an element given on the periodic table
Planetary Model: idea that an atom looks like the solar system, with electrons orbiting around the
nucleus. (the Rutherford experiment supported this model)
Plum Pudding Model: idea that the atom was positively charged, with electrons sprinkled throughout it.
The Rutherford experiment suggested that this model was inaccurate.
Mass: how heavy something is. An atom’s mass is made up of protons and neutrons’ masses
Volume: how much space something takes up. Electrons make up most of an atom’s volume
Level 3 Practice Questions
1. A) Write an equation that shows how to figure out how many neutrons an atom has.
Neutrons= mass- protons
B) Explain why the equation makes sense.
This makes sense because protons and neutrons are the heaviest subatomic particles. Mass of protons+
mass of neutrons= mass of nucleus (where an atom gets most of its weight). Electrons are not included
in the equation because electrons do not contribute to an atom’s mass.
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2. Fill in the chart.
Chemical
Symbol
P
Na+
Li—8
Protons
Neutrons
Electrons
Atomic #
Mass #
Net Charge
15
11
3
16
12
5
15
10
3
15
11
3
31
23
8
0
+1
0
Level 4 Practice Questions
1. Rutherford designed an experiment to see whether an atom looked like the solar system or
plum pudding. In his experiment, Rutherford shot gold atoms with a positively charged particle
beam.
Write a hypothesis for what would have happened in the experiment if Rutherford used a negatively
charged particle beam instead. (try to follow the 4 hypothesis rules that we learned in class!)
If the atom is shot with a negative particle beam, then the beam will deflect from electrons orbiting
the outside of the atom.
OR
If the atom is shot with a negative particle beam, then the beam will attract to the nucleus in the
center, and will not exit the atom.
2. Some atoms are more likely to gain electrons and become negatively charged ions. Some atoms
are more likely to lose electrons and become positively charged ions. Using what you know
about what an atom looks like, explain why you think this is true. (hint: think about the charges
of protons and electrons!)
Atoms with more protons have a stronger positive charge in their nucleus. This positive charge can
attract the negatively charged electrons from other atoms. Atoms with few protons in their nucleus
cannot attract electrons as well, and might lose their electrons.