Playing with Predictions
REAL JEOPARDY
A new element is found to have 12 energy levels (wow), and 8 valence electrons. It would be predicted to have the same type of properties as this group.
What are...
THE NOBLE GAS FAMILY, GROUP 18
REAL JEOPARDY
Carbon-13 has this many neutrons
What is ...
7
REAL JEOPARDY
Magnesium is likely to do this in order to follow the Octet Rule.
What is...
LOSE 2 ELECTRONS, or FORM a +2 ION
REAL JEOPARDY
Elements in the same group have similar chemical properties because of this.
What is...
THE SAME NUMBER OF VALENCE ELECTRONS
REAL JEOPARDY
Chlorine atoms need one more electron to fill their outer shell, so they are likely to do this in chemical reactions.
What is gain electrons or become negatively charged
A sample of element Z has 35 protons and 45 neutrons. Another sample of element Z has 35 protons and 46 neutrons. Evaluate how these two samples would differ in their chemical and physical properties.
a. They would have identical chemical properties but slightly different physical properties like density
b. They would have different chemical properties because the extra neutron changes the electron configuration
c. They would have different chemical properties but identical physical properties
d. They would have completely different chemical and physical properties because they are different elements
a. They would have identical chemical properties but slightly different physical properties like density
REAL JEOPARDY
If an atom gained or lost electrons to have a full outer shell, it would become this and could bond with other atoms.
What is ...
an ION
REAL JEOPARDY
A new element is discovered and it has 8 energy levels and 1 valence electron, it would be placed in this group.
What is ...
GROUP 1, The Alkali Metals
REAL JEOPARDY
If you discovered a new element with 119 protons, you could predict its properties by looking at this element on the periodic table, which is directly above it.
What is....
POTASSIUM
A chemist is analyzing an unknown element. It has 6 protons, 7 neutrons, and 6 electrons. Another sample has 6 protons, 8 neutrons, and 6 electrons. What conclusion can the chemist draw about these samples?
a. They are different elements with similar chemical properties
b. They are the same element with different physical properties
c. They are isotopes of carbon with different nuclear stability
d. They are isotopes of carbon that will have identical chemical behavior
c. They are isotopes of carbon with different nuclear stability
The atomic number tells us the number of protons in an element. Construct an explanation for why this single piece of information is sufficient to identify an element and predict many of its properties.
a. The atomic number determines the element's position on the periodic table, which follows predictable patterns
b. The atomic number directly determines an element's reactivity regardless of other factors
c. The atomic number tells us how many neutrons are in the nucleus, which determines stability
d. The atomic number is actually insufficient, and we need both atomic number and mass to identify elements
a. The atomic number determines the element's position on the periodic table, which follows predictable patterns
Hydrogen appears in group 1 of the periodic table but exhibits properties that sometimes resemble group 1 elements and sometimes resemble group 17 elements. Construct an explanation for why hydrogen doesn't fit perfectly into either group.
a. Hydrogen's unique position as the first element means it has properties of both metals and nonmetals
b. Hydrogen can either lose one electron like group 1 elements or gain one electron like group 17 elements
c. Hydrogen was mistakenly placed in group 1 and should actually be in its own special category
d. Hydrogen exhibits different properties because it has an incomplete outer energy level
b. Hydrogen can either lose one electron like group 1 elements or gain one electron like group 17 elements
When examining the periodic table, you notice that atomic radius generally decreases from left to right across a period. Develop a model that explains this trend based on atomic structure.
a. The decreasing trend occurs because elements on the right have fewer energy levels
b. The decreasing trend occurs because elements on the right have more protons but the same number of energy levels
c. The decreasing trend occurs because elements on the right have fewer electrons
d. The decreasing trend occurs because elements on the right have more neutrons pulling electrons inward
b. The decreasing trend occurs because elements on the right have more protons but the same number of energy levels
Carbon-12 and carbon-14 are isotopes used in different applications. Carbon-14 is radioactive and used in dating organic materials, while carbon-12 is stable. Analyze why these isotopes have different stability despite being the same element.
a. Carbon-14 has too many protons, making it unstable
b. Carbon-14 has too many electrons, disrupting its electron configuration
c. Carbon-14 has too many neutrons relative to its protons, creating nuclear instability
d. Carbon-14's instability is due to its position on the periodic table, not its isotopic nature
c. Carbon-14 has too many neutrons relative to its protons, creating nuclear instability
As you move down Group 1 (alkali metals), reactivity with water increases. Design a model that explains this trend based on atomic structure and periodic patterns.
a. Lower elements have more protons, increasing their attraction to water molecules
b. Lower elements have larger atomic radii, making their valence electrons easier to remove
c. Lower elements have more neutrons, making their nuclei more stable during reactions
d. Lower elements have more energy levels, allowing for more complex bonding with water
b. Lower elements have larger atomic radii, making their valence electrons easier to remove
The periodic table organizes elements into metals, nonmetals, and metalloids. Create a scientific argument for why silicon is classified as a metalloid rather than a metal or nonmetal.
a. Silicon was arbitrarily classified as a metalloid because it didn't fit neatly into either category
b. Silicon exhibits some properties of both metals and nonmetals due to its electron configuration
c. Silicon's position between metals and nonmetals on the table automatically makes it a metalloid
d. Silicon is actually misclassified and should be considered a nonmetal based on its properties
b. Silicon exhibits some properties of both metals and nonmetals due to its electron configuration
The mass number of an element is 35, and it has 18 neutrons. Using the periodic table patterns, predict this element's chemical behavior and justify your reasoning.
a. It would behave like a noble gas because it has a full outer electron shell
b. It would behave like a halogen because it needs one more electron to complete its outer shell
c. It would behave like an alkali metal because it has one valence electron
b. It would behave like a halogen because it needs one more electron to complete its outer shell
Hydrogen has a mass number of 1 and typically has 0 neutrons. Deuterium is an isotope of hydrogen with 1 neutron. Evaluate how the physical properties of water made with deuterium (heavy water) would differ from regular water, and explain why.
a. Heavy water would have identical properties because isotopes have identical chemical behavior
b. Heavy water would have a higher boiling point due to stronger hydrogen bonding from the added neutron mass
c. Heavy water would have a lower density because the extra neutron disrupts hydrogen bonding
d. Heavy water would have different color and taste because the neutron changes the electron configuration
b. Heavy water would have a higher boiling point due to stronger hydrogen bonding from the added neutron mass
A student notices that some elements in the periodic table don't follow the expected patterns. For example, copper has an electron configuration that differs from what would be predicted based on its position. Formulate an explanation for why such exceptions exist.
a. These elements were discovered later and forced into the table in available spaces
b. These elements have unique nuclear structures that affect their electron configurations
c. These elements experience special stability with certain electron configurations
d. These elements were incorrectly measured when the periodic table was being developed
c. These elements experience special stability with certain electron configurations
A sample contains atoms with 12 protons. After analyzing its properties, you find it reacts vigorously with water. However, when you analyze another sample with 12 protons, it reacts much more slowly with water. Develop a hypothesis that explains this observation.
a. The samples must be different elements that were misidentified
b. The samples must contain different isotopes of magnesium with different reaction rates
c. The samples must have different physical forms (powder vs. solid chunk) affecting surface area
d. The samples must have different numbers of electrons, creating ions with different reactivity
c. The samples must have different physical forms (powder vs. solid chunk) affecting surface area