Ch. 1 S And P Block Elements (Topic 13.2 And 13.3)

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  • 1/15 Questions

    The ionic radii of alkali metals will ___________ as we move down the group

    • Decrease
    • Increase
    • Remain same
    • First increase then decrease
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About This Quiz

This quiz covers key concepts of s and p block elements from Ch. 1, focusing on properties of alkali metals and the electronegativity of fluorine. It assesses understanding of ionic radii, ionization energies, and uses of flame tests in detecting metal salts.

Ch. 1 S And P Block Elements (Topic 13.2 And 13.3) - Quiz

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  • 2. 

    The property of alkali metals to give colouration in the burner flame has been used to detect their presence in salts by a test, known as

    • Slat analysis 

    • Chemical test

    • Flame test

    • Colour test

    Correct Answer
    A. Flame test
    Explanation
    The property of alkali metals to give coloration in the burner flame is utilized in the flame test. This test is used to detect the presence of alkali metals in salts. When the salt is heated in the flame, the metal ions present in the salt emit characteristic colors. Each alkali metal produces a unique color in the flame, allowing for the identification of the metal present. Therefore, the flame test is commonly used in salt analysis to identify and distinguish alkali metals.

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  • 3. 

    The electronegativity value of fluorine is 

    • 2

    • 3

    • 4

    • 5

    Correct Answer
    A. 4
    Explanation
    The electronegativity value of fluorine is 4. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Fluorine is the most electronegative element on the periodic table, with an electronegativity value of 4. This means that fluorine has a strong ability to attract electrons towards itself when forming a bond with another atom.

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  • 4. 

    Golden - yellow flame colour is shown by; 

    • Cu

    • Ba

    • Na

    • Li

    Correct Answer
    A. Na
    Explanation
    The golden-yellow flame color is shown by sodium (Na). When sodium is heated, it absorbs energy and its electrons become excited. As the electrons return to their ground state, they release energy in the form of light. The specific wavelength of light emitted by sodium corresponds to the golden-yellow color. This phenomenon is utilized in flame tests to identify the presence of sodium in compounds.

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  • 5. 

    Which alkali metal is comparitively harder?

    • Cs

    • Rb

    • K

    • Li

    Correct Answer
    A. Li
    Explanation
    Li is the correct answer because it is the alkali metal that is comparatively harder. Alkali metals are known for being soft and having low hardness, but among them, Li is the hardest. This is due to its smaller atomic radius and higher ionization energy compared to the other alkali metals. These factors contribute to stronger metallic bonding in Li, making it harder than the rest.

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  • 6. 

    Which alkali metal nitrate decomposes on heating?

    • NaNO3

    • LiNO3

    • KNO3

    • RbNO3

    Correct Answer
    A. LiNO3
    Explanation
    LiNO3 decomposes on heating because lithium nitrate is thermally unstable and breaks down into lithium oxide, nitrogen dioxide, and oxygen gas. This decomposition reaction is exothermic and occurs at a relatively low temperature compared to other alkali metal nitrates.

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  • 7. 

    Which nitride is volatile? 

    • Be3N2

    • Mg3N2

    • Ca3N2

    • Sr3N2

    Correct Answer
    A. Be3N2
    Explanation
    Be3N2 is the correct answer because beryllium nitride (Be3N2) is a highly volatile compound. Volatility refers to the tendency of a substance to vaporize or evaporate at a low temperature. In the case of Be3N2, the beryllium and nitrogen atoms are held together by weak bonds, making it easier for the compound to break apart and form a gas. This high volatility makes Be3N2 more likely to exist as a gas rather than a solid at room temperature.

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  • 8. 

    Which gas is evolved when metal carbonates are decomposed?

    • Oxygen

    • Hydrogen

    • Carbon dioxide

    • Nitrogen

    Correct Answer
    A. Carbon dioxide
    Explanation
    When metal carbonates are decomposed, carbon dioxide gas is evolved. This is because metal carbonates contain carbon and oxygen atoms bonded together. During decomposition, the heat breaks the bonds between the carbon and oxygen atoms, releasing carbon dioxide gas as a byproduct.

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  • 9. 

    The densities of alkali metals are quite low due to

    • The large atomic volume

    • The large atomic size

    • The large atomic radii

    • All of these 

    Correct Answer
    A. All of these 
    Explanation
    The densities of alkali metals are quite low because they have a large atomic volume, large atomic size, and large atomic radii. These factors contribute to the low packing efficiency of alkali metals, meaning that the atoms are more spread out and occupy a larger space. As a result, the mass of alkali metals is spread out over a larger volume, leading to lower densities.

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  • 10. 

    Why is the second ionization energy grater than first ionization energy? 

    • Because electron is weakly held

    • Distance of electron from the nucleus increases

    • Because of inert pair effect

    • Because of increasing nuclear pull

    Correct Answer
    A. Because of increasing nuclear pull
    Explanation
    The second ionization energy is greater than the first ionization energy because of increasing nuclear pull. This means that as an electron is removed from an atom, the remaining electrons experience a stronger attraction from the positively charged nucleus. This increased attraction makes it more difficult to remove a second electron, resulting in a higher ionization energy.

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  • 11. 

    The melting and boiling points of alkali metals  are very low because of the presence of

    • Weak inner atomic bonds in the solid state of the alkali metals

    • Weak Vander Waal's forces in the solid state of the alkali metals

    • Weak inner ionic bonds in the solid state of the alkali metals

    • Weak covalent bonds in the solid state of the alkali metals

    Correct Answer
    A. Weak inner atomic bonds in the solid state of the alkali metals
    Explanation
    The melting and boiling points of alkali metals are very low because of the presence of weak inner atomic bonds in the solid state of the alkali metals. This is because alkali metals have one valence electron, which is loosely held and easily lost. As a result, the metallic bonds between atoms are weak, leading to low melting and boiling points.

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  • 12. 

    Chemical formula of sodium nitrite is;

    • NaNO3

    • NaNO

    • NaNO2

    • Na2NO2

    Correct Answer
    A. NaNO2
    Explanation
    The correct answer is NaNO2. Sodium nitrite is a compound composed of one sodium atom (Na) and one nitrite ion (NO2-). The chemical formula represents the elements and the ratio of atoms in the compound, and NaNO2 accurately represents the composition of sodium nitrite.

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  • 13. 

    Formula of barium peroxide is;

    • Ba2O

    • BaO2

    • Ba2O2

    • BaO

    Correct Answer
    A. BaO2
    Explanation
    The formula of barium peroxide is BaO2. This is because the compound contains one barium ion (Ba2+) and two oxygen ions (O2-), resulting in the formula BaO2. The subscript 2 in O2 indicates that there are two oxygen ions present in the compound.

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  • 14. 

    Which concentrated is used to carry out flame test?

    • H2SO4

    • HNO3

    • H3PO4

    • HCl

    Correct Answer
    A. HCl
    Explanation
    HCl is the correct answer because it is commonly used in flame tests. Flame tests are used to identify the presence of certain metal ions in a compound. When a metal ion is heated in the flame, it emits a characteristic color. HCl is often used as the acid to dissolve the compound and provide the metal ion for the flame test. It helps in the dissociation of the metal ion, allowing it to release energy in the form of light when heated.

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  • 15. 

    Rb burns with _____________flame 

    • Red 

    • Reddish-violet

    • Lilac

    • Both a and b

    Correct Answer
    A. Both a and b
    Explanation
    Rb (Rubidium) burns with both a red and reddish-violet flame. The color of the flame depends on the temperature and the presence of other elements. At lower temperatures, Rubidium burns with a red flame, while at higher temperatures, it produces a reddish-violet flame.

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  • Mar 15, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Jul 16, 2020
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    Nuzhatibrahim1
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