Download BEAT_Sheet_for_Atoms_2016_ACA_answers

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BEAT Chemistry! (BE Able To): Atoms
 What is important to know about Dalton’s Atomic theory?
All matter is made up of tiny particles know as atoms
Dalton did not know about isotopes
Dalton did not know about subatomic particles (he thought the atom
was indivisible
 Describe the subatomic particles, including their properties, how and when they
were discovered, and where they are located
Proton
Positive (p+)
Neutron
No Charge (0)
Electron
Negative (e-)
Location in
atom
Nucleus
Nucleus
Electron cloud
Who discovered
particle
Rutherford
Chadwick
Thomson
Charge
 Explain Rutherford's Gold Foil Experiment, J.J. Thomson plum pudding model,
Dalton’s model, Bohr’s model, and the Quantum Mechanical Model. Explains any
experiments run and conclusions drawn from each experiment. Refer to your
notes and homework.
Daltons
Model
Said that all
elements are
made up of tiny
indivisible (not
able to be
divided)
particles called
atoms. Gave
testability to
atomic theory.
His model was
basically a
sphere.
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Thomson’s Model
Used Cathode
Ray Tube
experiment to
find that there
are subatomic
particles. He is
credited with
discovering the
electron. Later
had the Plum
Pudding Model
that suggested
all positive and
negative
particles are
jumbled up
together.
Rutherford’s
Model
Niels Bohr Model
Quantum
Mechanics Model
Gold Foil
Experiment
showed that
atoms are mostly
empty with a
small, dense,
positive nucleus.
Disproved
Thomson’s Plum
Pudding Model
Atoms consist of
electrons circling
in definite orbits
around a positive
nucleus.
Current atomic
theory. Atoms
are composed of
electrons in an
electron cloud
around the
nucleus.
 Fill in the table below
Element
Atomic
Number
Mass
Number
Atomic
Mass
Protons
Electrons
Neutron
Hyphen
notation
Indium
49
115
114.82
49
49
66
Indium-115
Vanadium
23
51
50.9415
23
23
28
Vanadium-51
Vanadium
23
50
50.9415
23
23
27
Vanadium-50
Tin, Sn2+
50
119
118.71
50
48
69
Ion
 Define isotope and explain how isotopes are similar and different.
each of two or more forms of the same element that contain equal numbers of protons
but different numbers of neutrons. SAME PROTONS, DIFFERENT NEUTRONS
 Determine the number of protons, neutrons and electrons in isotopes written in
general format and hyphen notation.
Isotope
General
format
Number of
protons
Number of
electrons
Number of
neutrons
Mass Number
Ti-46
Ti-47
 In Tungsten-184, 184 represents the mass number. What does the mass number
tell us? The mass number tells us the number of protons and the number of
neutrons in an atom.
 Are the following atoms electrically neutral or do they carry a charge and represent
an ion?
Electrically neutral and why? OR
Charge on the ion and why
5 protons and 5
Neutral. The protons equal the electrons
electrons
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7 protons and 10
electrons
Negative (3-). The electrons are greater than the protons.
The atoms must have gained electrons at some point.
12 protons and 10
electrons
Positive (2+). The electrons are less than the protons. The
atoms must have lost electrons at some point.
Circle the following which are isotopes of each other.
7
3𝑋
6
3𝑋
6
4𝑋
8
3𝑋
Mole Conversions:
A. What is the number of grams in 8 moles of Oxygen (O)?
8 moles O x 16 grams O
1
1 mole O
=
128 grams O
B. How many atoms are in 5 moles of Helium (He)?
5 moles He x 6.02 x 1023 atoms He
1
1 mole He
=
3.01 x 1024 atoms He
C. If you have 5.5 Kilograms of Hydrogen (H), how many atoms of Hydrogen do you
have? (Don’t forget to convert from kilograms to grams!)
5.5 kg x 1000 g = 5500 g H x 1 mole H x 6.02 x 1023 atoms H =3.31 x 1027 atoms H
1
1 kg
1
1gH
1 mole H
2016-2017