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All questions of Periodic Table for Year 10 Exam

How does the metallic character of elements change as you move across a Period on the Periodic Table from left to right?
  • a)
    It increases
  • b)
    It decreases
  • c)
    It remains constant
  • d)
    It fluctuates
Correct answer is option 'B'. Can you explain this answer?

Aurora Institute answered
The metallic character of elements diminishes as you progress across a Period on the Periodic Table from left to right. This trend occurs because atoms have a greater tendency to accept electrons to achieve a full valence shell rather than losing them to attain a full outer shell. Metals are predominantly situated on the left side of the Periodic Table, while non-metals are more common on the right side. This change in metallic character is a fundamental concept in understanding the properties and behavior of elements in the periodic table.
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Which group of elements on the Periodic Table is known for its rapid reactivity with water?
  • a)
    Group II
  • b)
    Group V
  • c)
    Group VII
  • d)
    Group I
Correct answer is option 'D'. Can you explain this answer?

Aurora Institute answered
Group I elements, also known as alkali metals, are recognized for their rapid reactivity with water. When alkali metals come into contact with water, they vigorously react, producing hydrogen gas and forming alkaline solutions. This reactivity increases as you move down the group, with cesium (Cs) being the most reactive alkali metal.

What property trend can be observed as one moves down Group I of the Periodic Table?
  • a)
    Melting point decreases
  • b)
    Boiling point increases
  • c)
    Density decreases
  • d)
    Reactivity increases
Correct answer is option 'A'. Can you explain this answer?

Aurora Institute answered
As one moves down Group I of the Periodic Table, the melting point of elements in this group decreases. This trend is a result of the increase in atomic size and the weakening of metallic bonds as you move down the group. For example, lithium (Li) has a higher melting point compared to potassium (K) due to the differences in atomic structure and bonding.

What does the final notation in an element's electronic configuration signify?
  • a)
    The number of valence electrons
  • b)
    The number of protons in the nucleus
  • c)
    The atomic number of the element
  • d)
    The atomic mass of the element
Correct answer is option 'A'. Can you explain this answer?

Prepworks Coaching answered
The final notation in an element's electronic configuration signifies the number of outer electrons that the atom possesses, which indicates the number of valence electrons. Valence electrons are the electrons in the outermost shell of an atom and play a crucial role in determining the element's chemical properties and reactivity.

What trend is observed in the reactivity of Group I metals as we move down the group?
  • a)
    Reactivity decreases
  • b)
    Reactivity remains constant
  • c)
    Reactivity increases
  • d)
    Reactivity fluctuates
Correct answer is option 'C'. Can you explain this answer?

Aurora Institute answered
The trend observed in the reactivity of Group I metals as we move down the group is that reactivity increases. This means that metals like rubidium, caesium, and francium exhibit more vigorous reactions with air and water compared to lithium, sodium, and potassium. Understanding this trend helps predict the behavior of alkali metals within the group.

How do elements within the same group on the Periodic Table differ as you move down the group?
  • a)
    They have the same number of electron shells
  • b)
    They have the same number of valence electrons
  • c)
    Their atomic numbers increase
  • d)
    Each subsequent element adds a full shell of electrons
Correct answer is option 'D'. Can you explain this answer?

Aurora Institute answered
As you move down a group on the Periodic Table, each subsequent element adds a full shell of electrons. This results in elements within the same group having different numbers of electron shells, with each lower element adding an additional shell compared to the element above it. The addition of electron shells influences the element's atomic radius and other chemical properties.

Which group of elements typically exhibits higher density compared to Group I elements?
  • a)
    Group VII
  • b)
    Transition elements
  • c)
    Lanthanides
  • d)
    Alkali metals
Correct answer is option 'B'. Can you explain this answer?

Prepworks Coaching answered
Transition elements, located in the middle section of the Periodic Table, generally have higher densities compared to Group I elements. This is attributed to the presence of greater mass and more complex atomic structures within transition elements. The density of transition elements contributes to their various industrial applications, such as in manufacturing, construction, and technology.

How do elements in the same group on the Periodic Table typically behave chemically?
  • a)
    They have the same number of protons
  • b)
    They have similar atomic masses
  • c)
    They exhibit similar chemical properties
  • d)
    They have the same number of neutrons
Correct answer is option 'C'. Can you explain this answer?

Prepworks Coaching answered
Elements in the same group on the Periodic Table exhibit similar chemical properties due to having the same number of electrons in their outermost shell. This similarity arises from the way their outermost electrons interact with other elements, leading to comparable behaviors in chemical reactions and bonding characteristics.

What does the electronic configuration of an atom reveal about its position on the Periodic Table?
  • a)
    The number of protons in the atom
  • b)
    The number of occupied electron shells
  • c)
    The atomic mass of the atom
  • d)
    The number of neutrons in the atom
Correct answer is option 'B'. Can you explain this answer?

Aurora Institute answered
The electronic configuration of an atom reveals the number of occupied electron shells of the atom, which in turn indicates the period in which the atom is placed on the Periodic Table. Each notation in the electronic configuration represents the arrangement of electrons in different shells, providing insight into the atom's position within the periodic table based on the number of shells that are occupied.

What is a notable characteristic of noble gases in terms of their reactivity?
  • a)
    Highly reactive with water
  • b)
    Form compounds easily
  • c)
    Exist as diatomic molecules
  • d)
    Generally inert
Correct answer is option 'D'. Can you explain this answer?

Prepworks Coaching answered
Noble gases are characterized by their inertness, meaning they are generally unreactive under normal conditions. This is due to their stable electron configurations, which result in minimal tendencies to gain, lose, or share electrons to form compounds. Helium, neon, argon, krypton, xenon, and radon are all noble gases found in Group VIII of the Periodic Table.

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