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97 Cards in this Set
- Front
- Back
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms toggether
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chemical bond
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a chemical bond resulting from the sharing of an electron pair between two atoms
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covalent bonding
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the chemical bond resulting fom electrical attraction between large numbers of cations and anions
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ionic bonding
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a covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in the balanced distribution of electrical charge
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nonpolar covalent bond
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having an uneven distribution of charge
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polar
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a covalent bond in which the baonded atoms have an unequal attraction for the shared electrons
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polar-covalent bond
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the energy required to break a chemical bond and from neutral isolated atoms
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bond energy
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the distance between two bonded atoms at their minimal potential energy, that is, the average distance between two bonded atoms
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bond length
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a formula that indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numberical subscripts
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chemical formula
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a molecule containing only two atoms
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diatomic molecule
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a covalent bond produced by the sharing of two pairs of electrons between two atoms
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double bond
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an ellectron configuration notation in which only the valence electrons of an atom of a particular elements are shown, indicated by the dots placed around the element's symbol
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electron-dot notation
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a formula in which atomic symbols represent nuclei and inner shell electrons dot pairs or dashes between two atomic symbols represents electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent uncharged electrons
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Lewis structure
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a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
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lone pair
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a chemical compound whose simplest units are molecules
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molecular compound
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a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound
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molecular formula
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a neutral group of atoms that are held together by covalent bonds
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molecule
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a double or triple bond
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multiple bond
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chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its hightest occupied energy level
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octet rule
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the bonding in molecules or ions that cannot be correctly represented by a single Lewis Structure
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resonance
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a covalent bond produced by the sharing of one pair of electrons between two atoms
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single bond
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a formula that indicates the number and types of atoms present in a molecule and also shows the bonding arrangement of the atoms; a formulat that indicates the kind, number, arrangement, and bonds but not the unshared electron pair of the atoms in a molecule
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structural formula
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a covalent bond produced by the sharing of three pairs of electrons between two atoms
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triple bond
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a pair of electrons that is not involved in bonding and that belongs exclusivelt to one atom
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unshared pair
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the simplest collection of atoms from which an ionic compound's formula can be established
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formulat unit
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a compound composed of positive and negative ions that are combined so that the numbers of positive nad negative charges are equal
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ionic compound
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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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a charged group of covalencely bonded atoms
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polyatomic ion
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the ability of a substance to be drawn puled or extruded trhough a small opening to produce a wire
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ductibilty
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the ability of a substance to be hammered into sheets
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malleability
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chemical bonding that results from the attraction between metal atoms and the surrounding sea of electroons
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metallic bonding
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equal but opposite charges that are separated by a short distance
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dipole
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orbitals of equal energy produced by the combinatinos of two or more orbitals on the same atom
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hybrid orbitals
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a force of attraction between polar molecules
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dipole-dipole force
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the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies
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hybridization
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the intermolectular force in which a hydrogen atom that is bonded to a hightly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
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hydrogen bonding
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the force of attraction between molecules
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intermolecular force
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the uneven distribution of molecular charge
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molecular polarity
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in a chemical bond the link between atoms results from the attraction between electrons and
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nuclei
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a covalent bond consists of
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a shared electron pair
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if two covalently bonded atoms are identical the bond is identified as
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nonpolar covalent
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a covalent bond in which there is an unequal attraction for the shared electrons is
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polar
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atoms with a stron attraction for electrons they share with another atom exhibit
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high electronegativity
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bonds with between 5% and 50% ionic character are considered to be
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polar covalent
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a nonpolar covalent bond is likely to exist between
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two identical atoms
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the greater the electronegativity difference between two bonded atoms the greater the percentage of
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ionic character
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the electrons involved in the formation of a chemiucal bond are called
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valence electrons
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a chemical bond resulting from electronstatic attraction between positive and negative ions is called an
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ionic bond
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if the electrons involved in bonding spend most of the time close to one atom rather than the toher the bond is
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polar covalent
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a chemical bond that results from the electrostatic attraction between positive and negative ions is called an
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ionic bond
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if electrons involved in bondnig spend most of the time closer to one atom rather thatn the other the bond is
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polar covalent
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if a bond's character is more than 50% ionic if the electronegativity difference between the two atoms is greater than
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1.7
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a large difference in electronegativity between two atoms in a bond results in
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ionic bonding
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what happens when atoms bond with each other
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they creeate arrangements of matter that are more stable
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the type of bond that shares electrons
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covalent
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elements that lose electrons and form positive ions
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metals
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metal-nonmetal bond
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ionic
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elements that gain electrons and from negative ions
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nonmetals
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electrons in the outermost energy levels
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valence electrons
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type of bond that transfers electrons
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ionic bond
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this bond forms compounds with low melting points
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molecular
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nonmetal nometal bond
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covalent
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this bond forms crystalline compounds
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ionic bond
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an atom or ion with a full outer energy level has a
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octet
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when an atom of one element combines chemically with an atom of another element both atoms usually attain the stable highest energyy level configuratin of a
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noble gas
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in a molecule of fluprine the two shared electrons give each fluoroing atom ___ electrson in the outer energy level
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8
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in writing a lewis structure each nonmetal atom except hydrogen shuld be surrounded by
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8 electrons
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in writing a lewis structure the central atom is the
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least electronegative atom
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to draw the electron-dot symbols for each atom in a lewis structure one must know the
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number of valence lectrons in each atom
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nature favors chemical bonding because
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potential energy is minimized when atoms are bonded
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when atoms are drawn together by attractive forces their potential energy
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is decreased
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potential energy is at a minium when
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the repulsion between the like charges equal the attraction of the opposite charges
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atoms are drawn to each other because the electron-proton attraction
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is stronger than the electron-electron and proton-proton repulsions
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the molecular formula H20 indicates a molecule
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with two atoms of hydrogen bonded with one atom of oxygen
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the strength of attraction between charged particles depends on the distance between the atoms involved in the bonds. tf
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true
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the bond length is the distance between two bonded atoms at their maximum potential energy
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false
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the energy required to form a chemical bond between to neutral atoms is called bond energy
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false
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according to the octet rule chemical compounds tend to form so that each atom has an octet of electrons in tis hightes energy level
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true
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when the orbitals of the hydrogen atoms in a hydrogen molecule overlap the electron density between the nuclei decreases
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false
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in the formula for sodium chloride NaCl stands for one
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formula unit
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the chemical formula for an ionic compound represents the
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simplest ratio of the combined ions that gives neutrality
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in a crystal of an ionic compound, each catino is surrounded bby a number of
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anions
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in a crystal the valence electrons of adjacent ions
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neutralize each other
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compared to the neutral atoms involved in its formationthe crystal lattice that results is
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lower in potential energy
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which of the following is NOT a proprerty of an ionic compound
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vaporizes at room temp
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compared to ionic compounds molecular compounds have
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lower melting points
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the forces of attraction between molecules ina molecular compound are
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weaker than the forces of ionif bonding
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at room temperature most ionic compounds will be
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solids
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molecular compounds are ____ at room temperature
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completely gaseous
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which is true of ionic compounds
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the ions cannot move in the solid structure
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NaCl is a molecular compound
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false
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lattice energy is released when the ions in a crystal lattice are separated from each each otther
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false
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ionic compounds are electrical conductors in their molten staes
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true
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an ionic compound is compose dof independent netural elements that can be isolated from each other
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false
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the atoms in molecular compounds are held together by covalent bonds
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true
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calculating lattice energies helps chemists compare bond strentgths in ionic compounds
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true
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a polyatomic ion with a shortage of electrons has a positive charge
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true
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