Download Snakes and Ladders Gaming Instructions

www.stao.ca
Student Activity
Snakes and Ladders
Gaming Instructions
1. Randomly select a package from your teacher and place your die and player token within it. This package
includes all materials needed for the game, including the board itself, and Snakes/Ladders/Regular
envelopes containing question/answer cards.
2. Play the board game with a partner.
3. Each person rolls the die. The one who rolls the highest number starts the game.
4. The first person rolls the die and must first answer a “regular” question in order to move forward from Start.
5. The next person rolls the die and repeats step 4.
6. Continue taking turns rolling the die and answering a question from the correct envelope.
7. If you arrive at the bottom of a ladder, you can only climb up it if you correctly answer a difficult Ladder
question. Place used “ladder” cards below card pile only if the questions were correctly answered. If not,
the next person who lands at the base of a ladder has an opportunity to answer a previously attempted
but incorrectly answered question.
8. If you arrive at the top of a snake, you must correctly answer an easy Snake question in order to avoid
sliding down it. Place used “snake” cards below card pile only if the questions were correctly answered.
If not, the next person who lands at the top of a snake has an opportunity to answer a previously
attempted but incorrectly answered question.
9. If you are on a spot other than at the bottom of a ladder or the top of a snake, then you must answer
a moderately difficult Regular question in order to move forward on the board the correct number
of spaces according to what you roll from the die.
10. Once a winner is declared, you have the option of either playing the same game again (consider this
option if a number of questions were left unanswered and/or answered incorrectly) or swap board
games with another group that has finished its game. Be sure to place all items back into the envelope
(including player tokens and die) before exchanging envelopes between groups.
11. HAVE FUN!
www.stao.ca
Snakes (easy) — Question 1
Snakes (easy) — Answer 1
What element has a higher electronegativity, Sr or Br?
Br has a higher electronegativity than Sr.
Snakes (easy) — Question 2
Snakes (easy) — Answer 2
Which type of element can generally lose electrons most
easily? Metals, nonmetals, or metalloids?
Metals can generally lose electrons most easily.
Snakes (easy) — Answer 3
Define Effective Nuclear Charge.
Effective Nuclear Charge (ENC) is the apparent nuclear
charge as experienced by the outermost electrons of
an atom when shielding by the innershell electrons
is taken into account.
Snakes (easy) — Question 4
Snakes (easy) — Answer 4
Determine which of the following elements you would
expect to have the lowest first ionization energy
Li, Cs, H, He, Ba
Of the elements listed, Cs has the lowest first
ionization energy.
Snakes (easy) — Question 3
Snakes and Ladders – Page 2
www.stao.ca
Snakes (easy) — Question 5
Snakes (easy) — Answer 5
Which element has more electronegativity, Kr or As?
As has more electronegativity than Kr.
Snakes (easy) — Question 6
Snakes (easy) — Answer 6
Fill in the blank: When moving from left to right across
a period, atomic radius ____________ .
When moving from left to right across a period, atomic
radius decreases.
Snakes (easy) — Question 7
Snakes (easy) — Answer 7
Fill in the blank: Ionization energy ____________ decreases
when going down a group.
Ionization energy decreases when going down a group.
Snakes (easy) — Question 8
Snakes (easy) — Answer 8
Which group of elements typically has comparatively higher
electron affinities, metals or non-metals?
Non-metals.
Snakes and Ladders – Page3
www.stao.ca
Snakes (easy) — Question 9
Snakes (easy) — Answer 9
What element on the periodic table has the smallest
atomic size?
Helium has the smallest atomic size.
Snakes (easy) — Question 10
Snakes (easy) — Answer 10
What element on the periodic table has the largest
atomic size?
Francium has the largest atomic size.
Snakes (easy) — Question 11
Snakes (easy) — Answer 11
Which element has the greatest electronegativity?
Fluorine.
Snakes (easy) — Question 12
Snakes (easy) — Answer 12
Which atom has the larger atomic radius, Li or K?
K because it is below Li in the group.
Snakes and Ladders – Page 4
www.stao.ca
Snakes (easy) — Question 13
Snakes (easy) — Answer 13
Which atom, Ca or Ni, has the larger atomic radius?
Ca because it is more towards the left of the periodic table
and atomic radius decreases from left to right.
Snakes (easy) — Question 14
Snakes (easy) — Answer 14
Which atom, Ga or B, has the larger atomic radius?
Ga because it is below B in the group.
Snakes (easy) — Question 15
Snakes (easy) — Answer 15
Which atom, O or C, has the larger atomic radius?
C because it is more towards the left than O in the period.
Snakes (easy) — Question 16
Snakes (easy) — Answer 16
Define nuclear charge.
Total positive charge associated with the nucleus, based on
the number of protons present.
Snakes and Ladders – Page 5
www.stao.ca
Snakes (easy) — Question 17
Snakes (easy) — Answer 17
Which element has the smallest atomic radius:
Na, Li, or Be?
Be has the smallest atomic radius because it is more
towards the right of the lower period.
Snakes (easy) — Question 18
Snakes (easy) — Answer 18
Which is larger, P 3- or S 2-?
P 3-
Snakes (easy) — Question 19
Snakes (easy) — Answer 19
What is atomic radius?
Atomic radius is one-half the distance between the nuclei
of two atoms of the same element, bondedor not bonded.
Snakes (easy) — Question 20
Snakes (easy) — Answer 20
Arrange this set of elements in order of increasing
ionization energy: F, Cl, Br
Br, Cl, F with F being the element with the highest
ionization energy.
Snakes and Ladders – Page 6
www.stao.ca
Ladder (hard) — Answer 1
Ladder (hard) — Question 1
Which is larger, F 1- or F and why?
F 1- is larger because the nuclear charge is unchanged,
but due to an extra electron, the electron-electron repulsion
increases causing the electron cloud to enlarge as would
be required to minimize this repulsion.
Ladder (hard) — Answer 2
Ladder (hard) — Question 2
Why does second ionization energy require more energy than
the first ionization energy?
Each successive ionization energy requires more energy to
remove a valence electron from an atom because after the first
ionization energy is supplied (first outer electron removed), there
is an increased nuclear pull from the nucleus (due to the presence
of a net positive charge with more protons than electrons present).
Electron-electron repulsion decreases and electrons are now
held more tightly than before. Trying to remove the second
electron will require more energy than the first because all the
extra energy goes towards overcoming the increased attraction
felt between the nucleus and second valence electron.
Ladder (hard) — Answer 3
Ladder (hard) — Question 3
Describe the relationship between ionization energy and
electronegativity.
If it takes more energy to remove an electron (ionization energy)
out of an atom, it means that the nucleus has a strong attraction
for outer electrons. The atom with a stronger attraction will
then attract shared electrons more strongly in whichever bond
it is involved with. Therefore, both properties show a positive
correlation (as one increases, so does the other).
Ladder (hard) — Answer 4
Ladder (hard) — Question 4
What is the periodic trend for ionic size across a period
and why?
Snakes and Ladders – Page 7
As you move from left to right for the metal side, effective
nuclear charge increases because there are more protons
than electrons. Thus, the valence electrons feel a stronger
pull towards the nucleus causing the valence electrons
to move closer to the nucleus, decreasing the ionic size.
However, ionic size increases as you move from left to
right for nonmetals because they tend to gain electrons
which will cause the electron-electron repulsion to increase,
making ionic size bigger.
www.stao.ca
Ladder (hard) — Answer 5
Ladder (hard) — Question 5
Why do noble gases have zero electron affinity?
Since noble gases have completely filled stable valence
shells, they do not want to gain electrons. Forcing noble
gases to accept an extra electron will cause an unstable
state for the atom.
Ladder (hard) — Answer 6
Ladder (hard) — Question 6
Why does ionization energy decrease as you go down
a group?
As you go down a group, a shell is added each time, and
this successively places valence electrons further away
from the nucleus. The valence electrons feel less attraction
for the nucleus and therefore, can be easily removed,
requiring less IE.
Ladder (hard) — Answer 7
Ladder (hard) — Question 7
How are ionization energy and electron affinity similar?
The trends involve absorbing and releasing of energies
when a valence electron is removed or added to an
atom, respectively.
Ladder (hard) — Question 8
Ladder (hard) — Answer 8
What are the three factors that affect atom radius?
The number of protons, number of energy levels and the
shielding effect.
Snakes and Ladders – Page 8
www.stao.ca
Ladder (hard) — Answer 9
Which is smaller, Na + or Na and why?
Na + is smaller because it has acquired a net positive charge
which increases the attraction between the nucleus and the
valence electrons (increase in ENC) while the shielding effect
stays constant causing the ionic radius to be smaller than
atomic radius.
Ladder (hard) — Question 10
Ladder (hard) — Answer 10
What does Coulomb's law say about attraction between
opposite charges?
Electrostatic force of attraction between opposite charges
decreases as the distance between them increases.
Ladder (hard) — Question 9
Ladder (hard) — Answer 11
Ladder (hard) — Question 11
What is the electron shielding effect?
Protons inside the nucleus attract the valence electrons.
Inner core electrons weaken this attraction between the
nucleus and the valence electrons. This effect is known
as the electron shielding effect.
Ladder (hard) — Answer 12
Ladder (hard) — Question 12
Why does electron shielding not change when going across
a period?
Snakes and Ladders – Page 9
Electron shielding does not change when going across
a period because the number of energy levels does not
change, only the number of valence electrons changes.
Therefore, there is no increase or decrease in the number
of inner core or kernel electrons, so electron shielding
remains the same throughout the period.
www.stao.ca
Ladder (hard) — Answer 13
Describe and explain the general trend for electronegativity
across a period.
Electronegativity of the atom increases from left to right.
This is due to the effective nuclear charge increasing as
you go across a period while electron shielding remains
the same. Therefore the attraction between the valence
electrons and the nucleus becomes stronger across a
period, causing atomic size to decrease. As atomic size
decreases, stronger attraction is felt between the nucleus
and shared electrons in a chemical bond as its outermost
shell is closer to the positively charged nucleus.
Ladder (hard) — Question 14
Ladder (hard) — Answer 14
Create an equation that incorporates the
first ionization energy.
X (g) + energy → X + + e -
Ladder (hard) — Question 13
Ladder (hard) — Answer 15
Ladder (hard) — Question 15
What is the difference between cations and anions?
Cations are formed when an atom loses its valence
electron(s) whereas anions are formed when an atom
gains valence electron(s).
Ladder (hard) — Question 16
Ladder (hard) — Answer 16
Order the following from smallest to largest atomic radius:
Fe, Ni, S, Ca, Li.
Li
Snakes and Ladders – Page 10
< S < Ni < Fe < Ca
www.stao.ca
Ladder (hard) — Question 17
Ladder (hard) — Answer 17
Create an equation that incorporates electron affinity.
X (g) + e - → X - (g) + energy
Ladder (hard) — Answer 18
Ladder (hard) — Question 18
What type of element will want to attract electrons and why?
Non-metals generally attract electrons easier than metals
as they seek to gain valence electrons in order to become
isoelectronic with the closest noble gas. Non-metals
generally have higher electron affinity and electronegativity
values than metals do. Therefore they have an easier ability
to gain or attract shared electrons.
Ladder (hard) — Answer 19
Give two reasons why potassium is bigger than magnesium.
Potassium is below magnesium on the periodic table and
therefore has more electron energy levels and more inner
core electrons, resulting in a greater electron shielding
effect. Another reason why potassium is larger is because
magnesium is placed further to the right on its period,
giving it a larger ENC value. With an increased effective
nuclear charge, the valence electrons in magnesium are
more strongly attracted to the nucleus. Therefore it has
a smaller atomic radius than potassium
Ladder (hard) — Question 20
Ladder (hard) — Answer 20
Why does fluorine have the highest electronegativity and
not helium, according to electronegativity trends?
All noble gases have an electronegativity of zero because
they have a full set of valence electrons therefore they
do not seek to share electrons with another atom.
Ladder (hard) — Question 19
Snakes and Ladders – Page 11
www.stao.ca
Regular (medium) — Question 1
Regular (medium) — Question 1
What group of elements primarily has an electron
affinity of zero?
The noble gases group has an electron affinity of zero.
Regular (medium) — Question 2
Regular (medium) — Question 2
Fill in the blank: The more energy released as a gaseous
atom accepts an electron, the ____________ its affinity
for an electron will be.
The more energy released as a gaseous atom accepts an
electron, the higher its affinity for an electron will be.
Regular (medium) — Question 3
Regular (medium) — Question 3
Define Effective Nuclear Charge.
The apparent nuclear charge, as experienced by the
outermost electrons of an atom, as a result of the
shielding by the inner-shell electrons.
Regular (medium) — Question 4
Regular (medium) — Question 4
Fill in the blank: Increased electron shielding results
in ____________ attraction for shared electrons by
the nucleus.
Increased electron shielding results in less attraction for
shared electrons by the nucleus.
Snakes and Ladders – Page 12
www.stao.ca
Regular (medium) — Question 5
Regular (medium) — Question 5
Define electronegativity.
Electronegativity is the measure of the attraction felt
by a nucleus of a bonded atom for shared electrons
in a chemical bond.
Regular (medium) — Question 6
Regular (medium) — Question 6
What are three factors that help explain the trends in the
periodic table?
Number of protons in the nucleus, number of energy levels,
the shielding effect.
Regular (medium) — Question 7
Regular (medium) — Question 7
Define ionization energy.
The amount of energy required to remove the outermost
electron from an atom or ion in the gaseous state.
Regular (medium) — Question 8
Regular (medium) — Question 8
Define electron affinity.
The energy typically released when an electron is added
to a neutral gaseous atom.
Snakes and Ladders – Page 13
www.stao.ca
Regular (medium) — Question 9
Regular (medium) — Question 9
Why is atomic size hard to measure?
It has no definite boundary.
Regular (medium) — Question 10
Regular (medium) — Question 10
Fill in the blank: Electron affinity and electronegativity
____________ when going from left to right, across
a period.
Electron affinity and electronegativity increase when going
from left to right across a period.
Regular (medium) — Question 11
Regular (medium) — Question 11
Which ion has the smaller ionic radius?
K + or Cs +
K+
Regular (medium) — Question 12
Regular (medium) — Question 12
Which ion, Al 3+ or P 3- , has the smaller
Al 3+
ionic radius?
Snakes and Ladders – Page 14
www.stao.ca
Regular (medium) — Question 13
Regular (medium) — Question 13
Which atom, Br or F, has the highest electronegativity?
F because it is above Br in the group.
Regular (medium) — Question 14
Regular (medium) — Question 14
Which atom has the highest first ionization energy:
Se , S or Te?
S because it is above Se and Te in the group.
Regular (medium) — Question 15
Regular (medium) — Question 15
Magnesium has a larger atomic radius than sodium
and beryllium. True or False?
False. Magnesium is smaller than sodium but bigger
than beryllium.
Regular (medium) — Question 16
Regular (medium) — Question 16
Helium has the greatest ionization energy and francium
has the lowest ionization energy. True or False?
True. Ionization energy increases across a period
and decreases down a group.
Snakes and Ladders – Page 15
www.stao.ca
Regular (medium) — Question 17
Regular (medium) — Question 17
Sulfur has a much lower electron affinity than calcium.
True or False?
False. Electron affinity increases across a period and
decreases down a group. Therefore, sulfur has a higher
electron affinity than calcium.
Regular (medium) — Question 18
Regular (medium) — Question 18
Which is most metallic? K, Rb, or Cs?
Cs
Regular (medium) — Question 19
Regular (medium) — Question 19
How is effective nuclear charge calculated?
nuclear charge + inner core charge
Regular (medium) — Question 20
Elements with three energy levels experience a weaker
shielding effect than elements with five energy levels
do. True or False?
Regular (medium) — Question 20
Snakes and Ladders – Page 16
False. Elements with five energy levels are bigger than
elements with three energy levels because they have more
inner core electrons that increase the shielding effect.