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GOB Chemistry Practice Final Exam Flashcards

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  • Characteristic NOT true for Group 1A (alkali metals)
    Most of them are liquids at room temperature is NOT true; they are solids.
  • Significance of significant figures
    They indicate the certain and estimated digits in a measurement.
  • Mass equivalent of 9.31 g
    9.31 g = 9310 mg.
  • Mass of 2.00 L glucose solution with density 1.15 g/mL
    Mass = 2.30 kg.
  • Electron configuration 1s2 2s2 2p6 3s2 3p5 corresponds to
    Element is chlorine (Cl).
  • Number of valence electrons in Group A element
    Equal to its group number.
  • Radiation type with highest energy
    Gamma rays have the highest energy.
  • Effect on mass number when a positron is emitted
    Mass number remains the same.
  • Half-life of a radioisotope
    Time it takes for one-half of the sample to decay.
  • Process in the Sun combining hydrogen nuclei
    Known as fusion.
  • Valence electrons location
    Located in the outermost energy level of an atom.
  • Number of valence electrons in carbon
    Carbon has four valence electrons.
  • Ion formation for sodium atom
    Sodium atom loses one electron to form an ion.
  • Number of electrons in ion with 20 protons and 2+ charge
    Ion has 18 electrons.
  • Correct formula for compound from Al and O
    Formula is \(Al_2O_3\).
  • Correct formula for iron(III) sulfide
    Formula is \(Fe_2S_3\).
  • Name of HSO4- ion
    Called hydrogen sulfate.
  • Polyatomic ion with 3- charge
    Phosphate ion has a 3- charge.
  • Element that does NOT exist as diatomic molecule
    Carbon does not exist as diatomic molecule.
  • Shape of carbon tetrachloride (CCl4) molecule
    CCl4 has a tetrahedral shape.
  • Ability of atom to attract shared electrons in covalent bond
    Called electronegativity.
  • Type of bond in HCl
    HCl contains a polar covalent bond.
  • Dipole direction in water molecule
    Negative portion points toward the oxygen atom.
  • Reason O-H bond in water is polar
    Because oxygen is more electronegative than hydrogen.
  • Overall polarity of molecule with symmetrical polar bonds
    Molecule is nonpolar.
  • Number of atoms on both sides of balanced chemical equation
    Number is the same on both sides.
  • Coefficient of H2 when balancing Al + H2SO4 → Al2(SO4)3 + H2
    Coefficient of H2 is 3.
  • Oxidized and reduced substances in Ba + Cl2 → BaCl2
    Ba is oxidized and Cl2 is reduced.
  • Substance reduced in redox reaction
    Substance reduced gains electrons.
  • Type of reaction: H2O2 → H2O + O2
    This is a decomposition reaction.
  • Avogadro's number represents
    Number of particles in 1 mole of a substance.
  • Molar mass of sodium phosphate (K3PO4)
    Molar mass is 164 g/mol.
  • Definition of molarity (M)
    Molarity is moles of solute per liter of solution.
  • Effect of increasing temperature on solubility of solid solute
    Usually increases solubility.
  • Henry's law states solubility of gas in liquid
    Increases as gas pressure above liquid increases.
  • Brønsted-Lowry definition of a base
    A base is a proton acceptor.
  • pH of solution with [H3O+] = 0.01 M
    pH = 2.0.
  • pH scale order from most basic to most acidic
    Order is 14, 10, 7, 4, 3, 1.