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    2rd periodical test in g9 science

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    99K views6 pages

    Quarterly Test in g9 Science 2nd Grading

    Uploaded by

    Rolly Miñon
    2rd periodical test in g9 science

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Flag for inappropriate content
    of 6

    Division of Romblon

    Romblon
    SECOND QUARTERLY TEST
    Grade 9 SCIENCE
    School Year 2016-2017
    Name: __________________________________Date: _____________________________
    Grade/Section: ___________________________
    _____________________________

    Score:

    ______________________________________________________________________________
    GENERAL DIRECTIONS: Read the sentences or questions carefully. Encircle
    the letter that corresponds to the best answer.
    1. Which type of bond is formed when an atom of sodium transfers an
    electron to an iodine atom?
    a. polar covalent
    c. metallic
    b. ionic
    d. nonpolar covalent
    2. When strontium reacts with oxygen to form strontium oxide, each
    strontium atom
    a. loses two ions
    c. loses two electrons
    b. gains two electrons
    d. gains two ions
    4. Which one of the following is most likely to be a covalent compound?
    a. Rb2S
    c. SrCl2
    c.
    b. CaO
    d.NCl3
    5. Which one of the following is most likely to be an ionic compound?
    a. NO2
    b.LiCl
    c.NaB
    d.SO
    6. Which pairs of atoms will share electrons when a bond is formed between
    them?
    a. Ba and I
    b. Li and I
    c. K and Cl
    d. C and O
    7. Which of these is a correct compound name?
    a. chloro hydride
    c. calcium bromine
    b. lead sodide
    d. argon sulfide
    8. A bond in which an atom contributes two electrons is:
    a. a double covalent bond c. a polar covalent bond
    b. an ionic bond
    d. a coordinate covalent bond
    9. A bond formed between two atoms in which each atom contributes a
    bonding electron is called a:
    a. polar bond
    c. coordinate covalent bond
    b. double covalent bond
    d. single covalent bond

    10. A covalent bond formed between two elements that have an


    electronegativity difference of 1.6 would be:
    a. a non polar bond
    c. moderately polar bond
    b. a very polar bond
    d. an ionic bond
    11. Which of the following molecules is polar?
    a. O2
    c. CO2
    b. Cl2
    d. HCl
    12. We would expect a bond formed between a silicon atom and an oxygen
    atom to be:
    a. an ionic bond
    c. a polar covalent bond
    b. a coordinate covalent bond d. a nonpolar covalent bond
    13. Which of the following is not a covalent compound?
    a. SCl2
    b. KCl
    b. c. HCl
    d. S2Cl2
    14. If a bonding pair of electrons is shared unequally between two atoms,
    the bond is:
    a. Ionic
    c. coordinate covalent
    b. nonpolar covalent
    d. polar covalent
    15. Electron Affinity is
    a. The energy required to remove an electron from an atom
    b. The measure of the ability of an atom in a chemical compound to
    attract electrons
    c. The energy change when an electron is acquired by a neutral
    atom
    d. The distance between radii of adjacent atoms
    16. Electronegativity is
    a. The energy required to remove and electrons from an atom
    b. The measure of the ability of an atom in a chemical compound to
    attract electrons
    c. The energy change when an electron is acquired by a neutral
    atom
    d. The distance between radii of adjacent atoms
    17. Ionization Energy is
    a. The energy required to remove an electron from an atom
    b. The measure of the ability of an atom in a chemical compound to
    attract electrons
    c. The energy change when an electron is acquired by a neutral
    atom
    d. The distance between radii of adjacent atoms
    18. Which element has the highest electronegativity?
    a. Fluorine
    c. iodine

    b. Lithium

    d. rubidium

    19. The letters s, p. d, or f are used to designate a particular______ within


    an energy level.
    a. sublevel,
    c. space
    b. Spin
    d. color.
    20. The space that may be occupied by a pair of electrons within a
    sublevel is a(n):
    a. Orbital
    c. Planks space
    b. Heisenbergs probability position.
    21. Electron affinity:
    a. energy needed to lose one electron from a compound,
    b. (b) energy needed to lose one electron,
    c. (c) energy needed to add an electron to a gaseous atom.
    22. Which of the following would correctly characterize a nonmetal?
    a. low ionization energy, low electron affinity
    b. high ionization energy, low electron affinity
    c. high ionization energy, high electron affinity
    d. low ionization energy, high electron affinity.
    23. When a metallic atom ionizes:
    a. it gains electrons,
    c. it loses electrons
    b. it neither gains nor loses electrons.
    24.
    The ___ have the lowest electronegativities.
    a. nonmetals
    c. metalloids
    b. metals
    25.
    The factor(s) that influence electronegativity is/are ____
    a. nuclear charge of the atom
    c. atomic radius of the atom
    b. the shielding effect
    d. all of the preceding.
    26. The ability to conduct electricity readily is a property of:
    a. nonmetals
    c. semiconductors
    b. metals
    d. halogens.
    27. 87. The particle that results when two or more atoms form covalent
    bonds is a:
    a. single charged atom
    c. atomic ion
    b. molecule
    28. 88. The strength of the bond between two atoms ___ as the difference
    in their electronegativities become larger.
    a. decreases
    c. increases
    b. remains constant
    d.could increase or decrease.

    29.

    compounds are normally solids at STP and tend to be soluble in water.


    a. Hydrogen
    c. metallic
    b. covalent
    d. Ionic.

    30.

    The London dispersion force is:


    a. attraction between positive and negative ions
    b. attraction between nonpolar molecules,
    c. attraction between polar molecules,
    d. measure of attraction for electrons.
    31.
    When two atoms combine by sharing electrons, where one has a
    bigger share, in order to obtain a stable octet they form a ___ bond.
    a. Ionic
    c.polar covalent
    b. non-polar covalent.
    32. When two atoms combine by transfer of electrons the opposite charges
    of the ions attract resulting in a____ bond.
    a. Ionic
    c. polar covalent
    b. non-polar covalent.
    33.
    What type of bond has an electronegativity difference of 3.1?
    a. Non-polar covalent
    c. Polar covalent
    b. Ionic
    d. Polar ionic
    34. The chemical bond formed when two atoms share one or more pairs of
    electrons is a(n)
    a. Ionic bond
    c. Orbital bond
    b. Polar bond
    d. Covalent bond
    35.
    Which of the following bonds are insoluble?
    a. ionic
    C. nonpolar covalent
    b. polar covalent
    D. none of the above
    36. Which of the following bonds are important in organic systems because
    they
    form chains of bonds that create organic molecules of life?
    a. ionic
    C. hydrogen
    b. polar covalent
    D. nonpolar covalent
    37.

    A bond in which an atom contributes two electrons is:


    a. a double covalent bond
    c. a polar covalent bond
    b. an ionic bond
    d. a coordinate covalent bond
    38. A bond formed between two atoms in which each atom contributes a
    bonding electron is called a:
    a. polar bond
    c. coordinate covalent bond
    b. double covalent bond
    d. single covalent bond

    39.

    The electron dot structure for hydrogen sulfide, H2S, is:


    a. H S
    c. H S
    b. b. H S H
    d. H H S

    40. A covalent bond formed between two elements that have an


    electronegativity difference of 1.6 would be:
    a. a nonpolar bond
    c. a moderately polar bond
    b. a very polar bond
    d. an ionic bond
    41. Which of the following is not a covalent compound?
    a. a. SCl2
    c. KCl
    b. HCl
    d. S2Cl2
    42. If a bonding pair of electrons is shared unequally between two atoms,
    the bond is:
    a. Ionic
    c. coordinate covalent
    b. nonpolar covalent
    d. polar covalent
    43. Which element has the abbreviated electron configuration, [Ar]
    4s2,3d10,4p6?
    a. Krypton
    c. Xenon
    b. Zinc
    d. Lead
    44. What is the total number of valence electrons in an atom with the electron
    configuration 2-8-5?
    a. 2
    c .5
    b. 8
    d. 15
    45. What term refers to the region of an atom where an electron is most likely to
    be found?
    a. quantum
    c. spectrum
    b. orbital
    d. orbit
    46. What is the total number of electrons in an Mg+2 ion?
    a. 10
    c. 24
    b. 2
    d. 12
    47.
    Which of the following bond(s) can be described as being weak and
    often transient
    electrical attractions between two atoms bearing partial electrical
    charges?
    a. ionic
    c. polar covalent
    b. nonpolar covalent
    d. all of the bove
    48. In the following molecular formula, how many of each atom is present?
    C6H12O6
    a. C = 6, H = 12, O = 6
    c. C = 12, H = 24, O = 12
    b. C = 1, H = 6, O = 12
    d. none of the above
    49.
    All atoms try to complete the number of ________ in their outer orbital.

    50.

    a. protons
    c. electrons
    b. neutrons
    d. all of the above
    Which of the following bonds are insoluble?
    a. ionic
    c. nonpolar covalent
    b. polar covalent
    d. none of the above

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