Chapter 6 – Chemistry Test Questions – Flashcards
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| A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds atoms together |
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| Chemical Bond |
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| Metals tend to _____ electrons and become _______; Nonmetals tend to _________ electrons and become _______ |
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| Lose/Cations;Gain/Anions |
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| Chemical bonding that results from the electrical attraction between cations and anions;give up electrons to other atoms |
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| Ionic Bonding |
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| Sharing of electron pairs between two atoms; electrons "owened" equally by bonded atoms |
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| Covalent Bonding |
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| How do you determine the type of bond? |
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| The difference in eectronegativity |
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| Bonding between two atoms of the same element is completely _______ |
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| Covalent |
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| Covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in balanced distribution of electrical charge |
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| Nonpolar-covalent bond |
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| Have uneven distribution of charge |
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| Polar |
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| Covalent bond in which the bonded atoms have unequal attraction for the shared electrons |
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| Polar-covalent bond |
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| 0-.3=_______ .3-1.7=________ 1.7-...=__________ |
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| Nonpolar-covalent;polar-covalent;ionic |
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| Neutral group of atoms that are held together by covalent bonds |
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| Molecule |
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| Chemical compound whose simplest units are molecules |
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| Molecular Compound |
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| Composition of a compound is given by the __________ ________ |
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| Chemical Formula |
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| Indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
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| Chemical Formula |
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| Shows the types and numbers of atoms combined in a single molecule of a molecualr compound |
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| Molecular Formula |
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| Molecule containing only two atoms |
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| Diatomic Molecule |
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| Potential energy ________ as the attraction gets stronger and _______ as the repulsion gets stronger |
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| Decreases;Increases |
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| Distance between two bonded atoms |
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| Bond Length |
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| Energy is ________ when bonded |
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| Released |
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| The energy required to break a chemical bond and form neutral isolated atoms |
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| Bond Energy |
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| As length _______ energy _______ and visa versa |
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| Increases;Decreases |
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| Chemical compounds tend to form so that each atom, by gaining, sharing, or losing electrons has an octet of electrons in its highest energy level |
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| Octet Rule |
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| Exceptions to the octet rule |
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| Boron can only have 6 VE;Expanded Valence(More than eight electrons esp. when bonded with F,O, or Cl) |
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| An electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol |
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| Electron-dot notation |
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| Pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
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| Unshared(Lone) pair |
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| Formulas in which atomic symbols represent nuclei and inner-shell electrons, dot pairs or dashes between two atomic symbols represent electron pairs in a covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
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| Lewis Structures |
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| A covalent bond in which one pair of electrons is shared between two atoms |
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| Single Bond |
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| Covalent bond in which two pairs of electrons are shared between two atoms, esp. C,N,O |
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| Double Bond |
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| Covalent bond in which three pairs of electrons are shared between two atoms |
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| Triple Bond |
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| ________ get shorter |
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| Stronger |
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| Bonding in molecules or ions that cannnot be correctly represented by a single lewis structure |
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| Resonance |
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| Composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal |
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| Ionic Compound |
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| Simplest collection of atoms from which an ionic compound's formula can be established |
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| Formula unit |
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| Ratio of ions in a compound depend on the _______ of the ions combined |
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| Charges |
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| Orderly arrangement in which ions are combined to minimize potential energy |
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| Crystal Lattice |
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| The energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
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| Lattice Energy |
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| Bond between molecules determine _______/_________ and ________ (Stronger equals ______) |
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| Melting point/boiling point and hardness;Higher |
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| Ionic compounds are ______ but ________ |
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| Hard but Brittle |
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| Ionic compounds are only conductors in _________ state or in ________ |
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| Molten/Water |
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| What two things are required for conductors |
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| Ions and movability |
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| A charged group of covalently bonded atoms |
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| Polyatomic ions(have characteristics of Molecular and ionic)...for lewis structures, if pos, subtract....if neg add |
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| Do not belong to any one atom but move freely about the metal's empty atomic orbitals |
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| Delocalized |
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| The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
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| Metallic Bonding |
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| Properties of metals(4) |
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| Good thermal/electrical conductors;Strong absorbers/reflectors of light |
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| Ability of a substance to be hammered into thin sheets |
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| Malleability |
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| Ability of a substance to be drawn through a small opening to produce wire |
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| Ductility |
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| The amount of energy absorbed as heat when a specified amount of a substance vaporizes at constant pressure |
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| Enthalpy(heat) of vaporization |
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| 5 bond sites 5 bonds |
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| triginal bipyramidal |
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| 5 bond sites 4 bonds |
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| seesaw |
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| 5 bond sites 3 bonds |
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| T shape |
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| 5 bond sites 2 bonds |
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| linear |
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| 6 bond sites 6 bonds |
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| octahedral |
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| 6 bond sites 5 bonds |
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| square base pyramid |
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| 6 bond sites 4 bonds |
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| square planar |
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| 3 bond sites 3 bonds |
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| triginal planar |
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| 4 bond sites 4 bonds |
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| tetrahedral |
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| 4 bond sites 3 bonds |
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| triginal pyramidal |
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| 4 bond sites 2 bonds |
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| bent |
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| 2 bond sites 2 bonds |
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| linear |
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| VSEPR stands for... |
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| Valance shell electron pair repulsion |
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| states that repulsion between the sets of valance electrons surrounding an atom causes these sets to be oriented as far apart as possible |
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| VSEPR theory |
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| The mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energy |
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| hybridization |
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| Intermolecular forces |
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| Dipole-dipole;Hydrogen;London dispersion forces |
