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Periodicity
By PAKAMAS TONGCHAROENSIRIKUL
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48 questions
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What does the periodic law state?
Properties of elements repeat periodically when arranged by atomic number
Elements in the same group have the same proton number
Elements are arranged by atomic mass
Elements' properties correlate with their electron configuration
Which elements have similar chemical properties?
Elements in the same group
Elements with the same atomic weight
Elements with the same atomic number
Elements in the same period
Which group on the periodic table is most reactive?
Group 8: Noble gases
Group 1: Alkali metals
Group 2: Alkaline earth metals
Group 17: Halogens
Which block of the periodic table contains the transition metals?
F-block
D-block
S-block
P-block
What block of the periodic table are the transition metals located in?
D-block
S-block
F-block
P-block
Which block of the periodic table contains elements with completely filled electron shells?
Halogens (P-block)
Alkali metals (S-block)
Noble gases (P-block)
Transition metals (D-block)
What group in the periodic table do lanthanides and actinides belong to?
S-block
D-block
F-block
P-block
In which block of the periodic table are group 1 alkali metals found?
D-block
S-block
F-block
P-block
What group in the Periodic Table contain the noble gases?
Group 18
Group 1
Group 17
Group 2
Why are noble gases unreactive?
They have no neutrons
They have less atomic mass
They have full electron shells
They lack protons
Which noble gas is used in 'neon' advertising signs?
Helium
Argon
Neon
Xenon
How many valence electrons does Neon (Ne) have?
6
7
2
8
What is the number of electrons of the outermost shell for noble gases?
2
6
4
8, excluding Helium
How many valence electrons does an atom in Group 17 have?
5
1
7
8
How many valence electrons does sulfur have?
8
7
2
6
Why do elements in the same group have similar chemical properties?
They have the same atomic number
They have the same number of valence electrons
They have the same atomic mass
They have the same number of energy levels
In terms of electron configuration, why is helium (He) considered a noble gas?
It has no valence electrons
It has a single energy level
Its outermost energy level is full
It has 8 valence electrons
Which group of the periodic table contains elements with two valence electrons?
Group 18
Group 1
Group 3
Group 2
What is the maximum number of valence electrons that an atom in s- or p-block can have in its outermost shell?
2
7
8
18
What happens to the atomic radius as you move from left to right across a period in the periodic table?
The atomic radius increases
The atomic radius remains constant
The atomic radius decreases
There is no discernable pattern
Which factor primarily causes the decrease in atomic radius across a period?
Increase in electron shielding
Decrease in electron-electron repulsion
Decrease in principal quantum number
Increase in effective nuclear charge
Why does atomic radius increase as you move down a group in the periodic table?
Additional energy levels are added, increasing the distance
More neutrons are added, increasing the radius
More protons are added, increasing the radius
More electrons are added, increasing the repulsion
Which of the following elements has the smallest atomic radius?
Hydrogen (H)
Neon (Ne)
Helium (He)
Lithium (Li)
What happens to the first ionization energy as you move down a group in the periodic table?
It stays the same
It decreases
It increases
It fluctuates unpredictably
What is the trend in atomic size as you move across a period from left to right?
There's no observable trend
Atomic size decreases
Atomic size increases
Atomic size stabilizes
Why does the ionization energy tend to increase as you move across a period from left to right?
Electrons are added to the same energy level
Atomic radius increases
Nuclear charge increases and atomic radius decreases
More energy levels are added
Which element would likely have the lowest first ionization energy?
Helium(He)
Oxygen(O)
Fluorine(F)
Francium(Fr)
An ion with 10 protons, 10 electrons and 11 neutrons is isoelectronic with what element?
Beryllium (Be)
Lithium (Li)
Boron (B)
Neon (Ne)
Why do elements in the same group on the periodic table have the same number of valence electrons?
They have the same number of protons
They have the same atomic number
They have the same atomic mass
They have the same outer electron configuration
What changes in an atom when it becomes a cation?
It loses electrons
It loses protons
It gains electrons
It gains neutrons
Which of the following elements is more likely to form a cation?
Nitrogen
Sodium
Fluorine
Oxygen
What effect does the loss of electrons have on the atomic size of a cation?
It has no effect on the atomic size
It decreases the atomic size
It oscillates the atomic size
It increases the atomic size
What charge does a cation carry?
None
Positive
Negative
Neutral
What happens to the atomic radius of an anion compared to its original atom?
It remains the same
It depends on the atom type
It becomes smaller
It becomes larger
Why does an atom form an anion?
It loses electrons to release energy
It wants to increase atomic radius
It gains electrons to reach stable energy levels
Atom cannot form anions
What charge does an anion carry?
Neutral charge
Negative charge
Both negative and positive charges
Positive charge
Which of the following elements is more likely to form an anion?
Helium
Argon
Neon
Fluorine
What does the electron shielding effect explain?
Decrease in atomic size down a group
Increase in atomic size across a period
Increase in ionization energy down a group
Decrease in electronegativity across a period
Which electron shell experiences the least shielding effect?
Last shell (farthest from the nucleus)
Second shell
Third shell
First shell (closest to the nucleus)
Why does electron shielding decrease ionization energy?
It increases the energy of the electrons
It decreases the energy of the electrons
Because it reduces the pull of the nucleus on electrons
Because it increases the pull of the nucleus on electrons
How does electron shielding affect atomic radius?
It causes the atomic radius to fluctuate
It has no effect on the atomic radius
It decreases the atomic radius
It increases the atomic radius
Why do the Noble Gases (Group 18) have low affinity to electrons?
They easily lose electrons
Their outer energy levels are already filled
They have small atomic radii
They have high ionization energy
Which element has the highest electronegativity?
Fluorine
Hydrogen
Oxygen
Nitrogen
How does electronegativity change across periods in the periodic table?
It decreases
It stays the same
There's no specific pattern
It increases
Why do atoms with higher electronegativities tend to attract bonding electrons?
They have more energy levels
They have stronger nucleus-electron attractions
They have more protons
They have a higher atomic mass
In bonding, which type of atom tends to receive electrons?
An atom with higher atomic mass
An atom with higher atomic number
An atom with higher electronegativity
An atom with lower electronegativity
Which chemical property is more closely associated with metals?
They tend to gain electrons
They are poor conductors of heat and electricity
They tend to lose electrons
They have low melting points
What is a characteristic property of nonmetals in the periodic table?
Usually good conductors of heat and electricity
Most are in the liquid state at room temperature
Generally poor conductors of heat and electricity
They tend to lose electrons easily