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      Atoms and Chemical Bonding on QuizRevolution

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      Atoms and Chemical Bonding

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      Atoms and Chemical Bonding
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      Which is not a factor affecting effective nuclear charge?
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       of players answered correctly.
      • the number of neutrons

      • the number of protons

      • the atomic radius

      • Screening Effect

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      Comments:
      1. Which is not a factor affecting effective nuclear charge?
        1. the number of neutrons
        2. the number of protons
        3. the atomic radius
        4. Screening Effect
      2. Why Ionisation Energy decreases slightly from Nitrogen to Oxygen?
        1. Because outermost electrons of O are in a higher subshell
        2. Because 4th electron added to O is opposite spin of the 3rd
        3. Because they are in different principal quantum shell
        4. Because they are in different subshell
      3. Isotopes of the same element have
        1. the same number of protons.
        2. the same number of neutrons.
        3. the same atomic mass
        4. the same number of megatrons.
      4. What is the shape of s orbital?
        1. Dumb-bell
        2. Spherical
        3. Circular
        4. Pyramid
      5. The number of orbitals in one principal quantum shell is determined by?
        1. n
        2. 2n^2
        3. n^2
        4. n+1
      6. What is the electronic configurations of Cr atoms?
        1. 1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1
        2. 1s2, 2s2, 2p6, 3s2, 3p6, 3d4, 4s2
        3. 1s2, 2s2, 2p6, 3s2, 3p6, 3d6
        4. 1s2, 2s2, 2p6, 3s2, 3p6, 3d4, 3f2
      7. In an ionic compound, how many cations are attracted to 1 anion and vice versa?
        1. 4
        2. 5
        3. 6
        4. 7
      8. The chemical properties of an element depend mainly on
        1. the number of neutrons
        2. the color of the element
        3. the number of protons and electrons
        4. the period of the element (in the periodic table of elements
      9. What is the relative mass of proton, neutron and electron respectively?
        1. 10, 1, 1/10
        2. 1, 10, 1840
        3. 1, 1, 1/1840
        4. 1840, 1, 1
      10. What are valence electrons?
        1. The no. of electrons in the outermost principal quantum shel
        2. The no. of electrons in the outermost subshell
        3. The no. of electrons in the outermost orbital
        4. The no. of electrons in an ionic compound
      11. Beryllium has a higher melting point than Magnesium because
        1. it is malleable
        2. magnesiums are inferior
        3. it has a higher charge density
        4. magnesium is less reactive than beryllium
      12. Which of the following metals is the most reactive?
        1. Fr
        2. K
        3. Li
        4. Na
      13. Which of the following correctly describe isotopes?
        1. same physical properties and chemical properties
        2. Differnt physical properties and chemical properties
        3. same neutron no. but different proton and electron no.
        4. same proton and electron no. but different neutron no.
      14. Where will the electrons travel to?
        1. Up
        2. Down
        3. Straight
        4. They will explode before they do

        1. Up down left right middle back KABOOM!

      15. Which of the following are true?
        1. Ionic compounds conduct electricity in all states
        2. Metals conduct electricity in all states
        3. Ionic compounds conduct electricity in solid state ONLY
        4. Metals conduct electricity in solid state ONLY
      16. How is Bromine-79 and Bromine-81 related?
        1. They are twins.
        2. Bromine-81 has 2 more electrons.
        3. Bromine-79 has more neutrons.
        4. They are isotopes.
      17. Ionisation energy (IE) is
        1. the power an ion possesses
        2. a term that does not exist
        3. the number of valence electrons
        4. the energy required to remove 1 mole of electron from atoms
      18. Why are metals malleable and ductile?
        1. Because they are hard
        2. Because they have + charge
        3. Because delocalized electrons can hold the cations together
        4. Because it contains metal cations
      19. Why ionic compounds have high melting and boiling points?
        1. They are widely spaced
        2. Electrostatic attraction very strong
        3. They are formed of 2 elements
        4. Heat is required to expand it
      20. The electronic configuration of Copper? (29 electrons)
        1. 1s2, 2s2, 2p6, 3s2, 3p2, 3d10,4s5
        2. 1s2, 2s2, 2p6, 3s2, 3p2, 3d10,4s1
        3. 1s2, 2s2, 2p6, 3s2, 3p6, 3d9,4s2
        4. 1s2, 2s2, 2p6, 3s2, 3p6, 3d10,4s1
      21. Why Ionisation Energy decreases down the group? (+ is increase, - is decrease)
        1. proton no. +, screening effect and atomic radius + more
        2. proton no. -,screening effect and atomic radius - more
        3. proton no. +, screening effect and atomic radius - more
        4. proton no. -, screening effect and atomic radius + more
      22. Which elements have no paired d-electrons in its ground state?
        1. Vanadium
        2. Iron
        3. Nickel
        4. Zinc
      23. Why chemical reactions only involve electrons?
        1. Because electrons tend to go to another atom
        2. Because electrons are not restricted
        3. Because electrons are light
        4. Because electrons can be shared, given out or taken in
      24. Which of the following is untrue for an ionic compound?
        1. it has ions
        2. it is brittle
        3. the bonds break and the compound explodes upon heating
        4. it does not conduct electricity in solid state
      25. What is the trend in the no. of valence electrons?
        1. Metals have many, non-metals have few
        2. Metals have few, non-metals have many
        3. Noble gases have few, other gases have many
        4. Noble gases have many, other gases have few
      26. The hydrogen atom does not contain :
        1. Electron
        2. Proton
        3. Neutron
        4. Principal Quantum Shell

        1. Congrats?

      27. The lower the principal quantum shell,
        1. the taller the electron
        2. the higher the first ionisation energy
        3. the more electricity it has
        4. the more electrons it has
      28. The crystal structure of ionic compounds consists of
        1. a giant 3D ionic lattice
        2. a spherical ionic lattice
        3. floating balls
        4. metal cations in a sea of delocalized electrons
      29. Aufbau's Principle states that
        1. electrons revolve around protons and neutrons
        2. the lowest energy levels are always filled first.
        3. electrons are lazy.
        4. pigs can fly too
      30. Atoms bond for
        1. fun
        2. stability
        3. more power
        4. more electrons

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