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WorksheetsExploring Atoms and Their Properties
Total questions: 24
Worksheet time: 31mins
Explain how the arrangement of electrons in an atom determines its position in the periodic table and its chemical properties.
The number of protons determines the position, while electrons have no effect.
The arrangement of electrons in shells and subshells determines the position and chemical properties.
The number of neutrons determines the position, while electrons determine chemical properties.
The atomic mass determines the position, while electrons determine chemical properties.
Analyze the trend in atomic radius as you move across a period from left to right in the periodic table. Explain the reasoning behind this trend.
Atomic radius increases due to the addition of more electron shells.
Atomic radius decreases due to increased nuclear charge pulling electrons closer.
Atomic radius remains constant because the number of protons and electrons are balanced.
Atomic radius increases due to increased electron-electron repulsion.
Compare and contrast ionic and covalent bonds in terms of electron transfer and sharing. Provide examples to support your explanation.
Ionic bonds involve sharing electrons, while covalent bonds involve transferring electrons.
Ionic bonds involve transferring electrons, while covalent bonds involve sharing electrons.
Both ionic and covalent bonds involve sharing electrons equally.
Both ionic and covalent bonds involve transferring electrons equally.
Scarlett and Mason are conducting an experiment to evaluate the impact of temperature on the states of matter. They focus on the transition between solid, liquid, and gas.
Increasing temperature always turns solids into gases directly.
Increasing temperature causes solids to melt into liquids and liquids to evaporate into gases.
Decreasing temperature causes gases to turn into solids directly.
Temperature has no effect on the states of matter.
Samuel and Abigail are discussing how isotopes of an element differ and how this affects the calculation of atomic mass.
Isotopes have different numbers of protons, affecting atomic mass.
Isotopes have different numbers of neutrons, affecting atomic mass.
Isotopes have different numbers of electrons, affecting atomic mass.
Isotopes have the same number of neutrons, not affecting atomic mass.
Predict how the electronegativity of elements changes as you move down a group in the periodic table and justify your prediction.
Electronegativity increases due to increased atomic size.
Electronegativity decreases due to increased atomic size.
Electronegativity remains constant because the number of electron shells is the same.
Electronegativity increases due to decreased atomic size.
Samuel is observing the behavior of particles in different states of matter. Analyze the relationship between the kinetic energy of particles and the state of matter they are in.
Particles in a solid have the highest kinetic energy.
Particles in a gas have the highest kinetic energy.
Particles in a liquid have the highest kinetic energy.
All states of matter have the same kinetic energy.
Aria and Grace are discussing why some elements are more reactive than others. Critically evaluate the role of valence electrons in determining the chemical reactivity of an element.
Valence electrons have no effect on chemical reactivity.
The number of valence electrons determines the element's ability to form bonds.
Valence electrons determine the element's atomic mass.
Valence electrons determine the element's color.
The periodic table is a chart that organizes the elements based on their atomic properties. Elements in the periodic table are organized according to the periodic law. The periodic law states that chemical and physical properties of elements are periodic functions of their atomic numbers (the number of protons in the nucleus). As the atomic number of elements increases, different elements display similar characteristics at regular intervals.
Periodic law states that elements are arranged _______________________________________________________________.
in alphabetical order.
from largest to smallest.
as periodic functions of their atomic numbers.
there is no rhyme or reason.
It stacks the elements in columns according to the number of valence electrons in an atom of the element. Valence electrons are those in the outermost shell of the atom and the ones that participate in reactions. The number of valence electrons is associated with the element’s reactivity. Elements with the same number of valence electrons behave in a similar way in reactions and so are grouped together in the same column on the periodic table.
What does the amount of valance electrons determine about an element?
Its row in the table.
Its atomic number.
Its atomic mass.
Its reactivity with other elements.
The maximum number of valence electrons an atom can have is eight, with the exception of helium, which can have only two. In each row, or period, of the periodic table, the last element on the right has the maximum number of valence electrons. Its outermost shell is full, and a new period in which the element on the far left has only one valence electron begins in the next row.
How do you determine how many valance electrons an element has?
Count how far over it is from the left in its row.
Count which row it is in.
They all have eight.
You can not determine this from the periodic table.
In the periodic table, similar elements are arranged in vertical columns called groups. Some of the major groups include Group 1: alkali metals; Group 2: alkaline earth metals; Group 17: halogens; and Group 18: noble gases. Elements within each group have similar properties and characteristic behaviors because of their similar numbers of valence electrons.
In what direction are groups arranged in the periodic table?
Side to side
Up and down.
Diagonally
In sections.
Alkali metals have 1 valence electron, making them highly reactive. With the exception of hydrogen, they tend to be very soft metals with low melting points. Examples include sodium and potassium.
Alkaline earth metals have 2 valence electrons and also are highly reactive and have high melting points. Examples include calcium and magnesium.
Halogens have 7 valence electrons and therefore are highly reactive. They tend to form compounds in nature. Examples include chlorine and fluorine.
Noble gases have a complete outer shell with 8 valence electrons, making them nonreactive. They are typically colorless, odorless gases. Examples include helium, neon, and argon.
Which group of elements tend to form compounds in nature?
Alkaline metals
Alkaline Earth metals
Halogens
Noble Gases
Alkali metals have 1 valence electron, making them highly reactive. With the exception of hydrogen, they tend to be very soft metals with low melting points. Examples include sodium and potassium.
Alkaline earth metals have 2 valence electrons and also are highly reactive and have high melting points. Examples include calcium and magnesium.
Halogens have 7 valence electrons and therefore are highly reactive. They tend to form compounds in nature. Examples include chlorine and fluorine.
Noble gases have a complete outer shell with 8 valence electrons, making them nonreactive. They are typically colorless, odorless gases. Examples include helium, neon, and argon.
Which group is highly reactive with high melting points?
Alkaline metals
Alkaline earth metals
Halogens
Noble gases
The periodic table is further arranged into three major regions, including the metals, metalloids, and non-metals. Metals are on the left of the table; they are shiny and flexible, conduct heat and electricity, and participate in ionic reactions. Non-metals are on the far right of the table; they are dull and brittle, are poor conductors, and typically participate in ionic reactions.
Which one is NOT a major region of elements in the periodic table?
Metals
Mettaloids
Non metals
Gases
atomic number
gas at room temperature, low boiling point
a subatomic particle that has a negative charge
number or protons and neutrons
the number of protons in the nucleus of an atom
period
Elements that occur in vertical columns on the periodic table.
A horizontal row of elements in the periodic table
Found in group two of the periodic table; highly reactive
A subatomic particle that has a negative charge
neutron
A subatomic particle that has a positive charge and that is found in the nucleus of an atom
not able to conduct heat or electricity, little to no metallic luster
A subatomic particle that has a negative charge
A small particle in the nucleus of the atom, with no electrical charge
A subatomic particle that has a positive charge and that is found in the nucleus of an atom
Proton
elecrtron
groups
neutrons
A subatomic particle that has a negative charge
nobles gases
protons
electrons
neutrons
Which correctly describes a Sodium (Na) atom?
Atomic Number- 16
Protons- 16
Electrons- 16
Mass- 32
Neutrons- 16
Atomic Number- 23
Protons- 23
Electrons- 23
Mass- 11
Neutrons- 11
Atomic Number- 11
Protons- 23
Electrons- 23
Mass- 23
Neutrons- 11
Atomic Number- 11
Protons- 11
Electrons- 11
Mass- 23
Neutrons- 12
Elements in the same ________ are more chemically similar.
group
period
club
table
Which element is similar to Mg?
Ca
B
What is the primary factor that determines the chemical reactivity of an element?
The number of protons in the nucleus.
The number of valence electrons.
The atomic mass of the element.
The number of neutrons in the nucleus.
