AQA A Level Chemistry - Molecules: Shapes & Forces

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Questions and Answers

Match the following types of electron pairs with their properties:

Lone pairs = Repel each other more than bonded pairs Bond pairs = Represent shared electrons between atoms Double bonds = Treated the same as single bonds in repulsion Triple bonds = Have greater repulsion than double bonds

Match the following VSEPR rules with their descriptions:

Valence shell electrons = Found in the outer shell of an atom Electron repulsion = Same charge repels other electrons Lone pair effect = Repels more than bonded pairs Stable shape = Adopted to minimize repulsion forces

Match the following shapes of molecules with the corresponding bonding scenarios:

Linear = 2 bonding pairs, 0 lone pairs Trigonal planar = 3 bonding pairs, 0 lone pairs Bent = 2 bonding pairs, 1 lone pair Tetrahedral = 4 bonding pairs, 0 lone pairs

Match the following pairs of electron interaction with their repulsion strength:

Lone pair - Lone pair = Strongest repulsion Lone pair - Bond pair = Intermediate repulsion Bond pair - Bond pair = Weakest repulsion Double bond - Double bond = Greater than single bonds Signup and view all the answers

Match the following terms related to electron pairs with their definitions:

Valence shell = Outermost shell of an atom Repulsion = Forces between like charges Concentrated charge cloud = Typically associated with lone pairs Molecule stability = Minimized repulsive forces between pairs Signup and view all the answers

Match the following terms with their specific roles in VSEPR theory:

Bonded pairs = Electrons shared between atoms Lone pairs = Electrons localized on a single atom Repulsive forces = Influence the molecular shape Electron pairs = Determine bond angles in molecules Signup and view all the answers

Match the following types of bonds with their interactions:

Single bond = One pair of shared electrons Double bond = Two pairs of shared electrons Triple bond = Three pairs of shared electrons Multiple bonds = Involve increased electron repulsion Signup and view all the answers

Match the following concepts related to molecular shape with their implications:

Electron pair arrangement = Affects molecular geometry Bond angles = Determined by electron pair repulsion Shape stability = Minimized repulsion leads to this VSEPR theory = Predicts shapes based on electron pairs Signup and view all the answers

Match the following types of electron pairs with their characteristics:

Lone pairs = Higher repulsive force Bonding pairs = Lower repulsive force Double bonds = Intermediate repulsive force Triple bonds = Higher repulsive force than single bonds Signup and view all the answers

Match the following molecules with their shapes:

CCl4 = Tetrahedral N(CH3)3 = Trigonal pyramidal Phosphorus(V) chloride = Trigonal bipyramidal CO2 = Linear Signup and view all the answers

Match the following bond angles with their corresponding molecular shapes:

Tetrahedral = $109.5^{ ext{o}}$ Trigonal planar = $120^{ ext{o}}$ Trigonal bipyramidal = $90^{ ext{o}}$ and $120^{ ext{o}}$ Linear = $180^{ ext{o}}$ Signup and view all the answers

Match the following groups with their number of valence electrons:

Group 15 = 5 valence electrons Group 17 = 7 valence electrons Group 14 = 4 valence electrons Group 16 = 6 valence electrons Signup and view all the answers

Match the following shapes with their molecular examples:

Trigonal bipyramidal = Phosphorus(V) chloride Tetrahedral = CCl4 Trigonal pyramidal = N(CH3)3 Linear = CO2 Signup and view all the answers

Match the following molecular shape descriptors with their definitions:

Lone pair = Non-bonding electron pair Bonding pair = Electron pair shared between atoms Electronegativity = Ability to attract electrons in a bond Molecular geometry = 3D arrangement of atoms in a molecule Signup and view all the answers

Match the following terms with their descriptions:

VSEPR = Theory to predict molecular shapes Covalent bond = Sharing of electron pairs between atoms Valence electrons = Electrons in the outermost shell Bond angle = Angle between two bonds in a molecule Signup and view all the answers

Match the following bond types with examples:

Single bond = C–H in methane Double bond = O=O in oxygen Triple bond = N≡N in nitrogen Polar covalent bond = H–Cl in hydrochloric acid Signup and view all the answers

Match the following elements with their characteristics regarding electronegativity:

Sodium = Higher electronegativity than caesium Caesium = Lower electronegativity than sodium Oxygen = Higher electronegativity than nitrogen Bromine = Lower electronegativity than chlorine Signup and view all the answers

Match the groups in the periodic table with their electronegativity trend:

Groups = Electronegativity decreases down the group Periods = Electronegativity increases across the period Transition Metals = Variable electronegativity Noble Gases = Generally low electronegativity Signup and view all the answers

Match the factor with its effect on electronegativity:

Increasing nuclear charge = Increases electronegativity Adding new electron shells = Decreases electronegativity Increasing atomic radii = Decreases electronegativity Constant shielding across a period = Increases electronegativity Signup and view all the answers

Match the statement with its implications for bonding:

High electronegativity = Strong attraction for bonding electrons Low electronegativity = Weak attraction for bonding electrons Increased shielding = Less attraction between nucleus and outer electrons Decreased shielding = Greater attraction between nucleus and outer electrons Signup and view all the answers

Match the following observations with their explanations:

Electronegativity trend in groups = Decreases due to increased shielding Electronegativity trend across periods = Increases due to higher nuclear charge Large atomic radii down a group = Due to more filled electron shells Small atomic radii across a period = Due to increased attraction between nucleus and electrons Signup and view all the answers

Match the type of electron to the corresponding shell configuration:

Outer electrons = Experience attraction from the nucleus Inner electrons = Shield the outer electrons Valence electrons = Participate in chemical bonding Core electrons = Do not participate in bonding Signup and view all the answers

Match the elements with their respective groups:

Sodium = Group 1 Chlorine = Group 17 Bromine = Group 17 Calcium = Group 2 Signup and view all the answers

Match the following types of bonds or forces with their descriptions:

Intramolecular forces = Forces within a molecule, usually covalent bonds Covalent bonds = Bonds formed by sharing outer electrons between atoms Intermolecular forces = Forces between molecules that are weaker than intramolecular forces Hydrogen bonding = A special type of permanent dipole - dipole force Signup and view all the answers

Match the following intermolecular forces with their characteristics:

Induced dipole - dipole forces = Also called van der Waals or London dispersion forces Permanent dipole - dipole forces = Attractive forces between neighboring molecules with a permanent dipole Hydrogen bonding = Stronger than standard dipole - dipole interactions Intermolecular forces = Weaker forces compared to intramolecular forces Signup and view all the answers

Match the following elements with their electronegativity trends:

Fluorine = Most electronegative element in the periodic table Electronegativity = Increases going across periods in the periodic table Top right of the periodic table = Region with highest electronegativity Electronegativity trend = General increase towards the top right corner Signup and view all the answers

Match the following bond types with their strength relative to each other:

Covalent bond = Stronger than hydrogen bonds Hydrogen bond = About one tenth the strength of covalent bonds Intramolecular forces = Stronger than intermolecular forces Intermolecular forces = Weaker than intramolecular forces Signup and view all the answers

Match the following types of covalent bonds with their characteristics:

Single bond = Involves one shared pair of electrons Double bond = Involves two shared pairs of electrons Triple bond = Involves three shared pairs of electrons Coordinate bond = Involves one atom donating both electrons Signup and view all the answers

Match the following definitions with the appropriate terms:

Intramolecular forces = Covalent bonds within a molecule Intermolecular forces = Attractive forces between different molecules Electronegativity = Tendency of an atom to attract electrons Lewis structures = Diagrams showing covalent bonds and molecule structure Signup and view all the answers

Match the following descriptions with the types of intermolecular forces:

Induced dipole forces = Temporary shifts in electron distribution in molecules Permanent dipole-dipole forces = Ongoing attractions between permanent dipoles Hydrogen bonding = Special strong interaction involving hydrogen atoms Dipole-induced dipole forces = One polar molecule inducing a dipole in another Signup and view all the answers

Match the following concepts related to electronegativity with their implications:

Increasing electronegativity = Represents increasing attraction for electrons Periodic table trends = Electronegativity increases across periods Fluorine's position = Indicates it has the highest electronegativity Atoms with higher electronegativity = Tend to attract electrons more strongly Signup and view all the answers

Match the type of bond with its characteristic:

Nonpolar bond = Electrons shared equally Polar bond = Electrons drawn toward more electronegative atom Permanent dipole = Always has a negative and positive charge end Asymmetric electron distribution = Charge centers do not coincide Signup and view all the answers

Match the term with its definition:

Electronegativity = Ability of an atom to attract electrons δ+ (delta positive) = Partial charge on less electronegative atom δ- (delta negative) = Partial charge on more electronegative atom Dipole-dipole forces = Attraction between polar molecules due to permanent dipoles Signup and view all the answers

Match the atom to its electronegativity characteristic:

Chlorine (Cl) = Higher electronegativity than hydrogen (H) Hydrogen (H) = Lower electronegativity than chlorine (Cl) Oxygen (O) = Significantly high electronegativity Carbon (C) = Moderate electronegativity compared to metals Signup and view all the answers

Match the concept with its effect:

Greater difference in electronegativity = More polar the bond Same electronegativities = Forms a nonpolar bond Permanent dipole = Induces attraction between molecules Asymmetry in electron distribution = Differentiates between polar and nonpolar bonds Signup and view all the answers

Match the term with its example:

Polar bond = HCl Nonpolar bond = Cl2 Permanent dipole = Water (H2O) Covalent bond = O2 Signup and view all the answers

Match the bond type with its electron behavior:

Nonpolar covalent bond = Equal sharing of electrons Polar covalent bond = Unequal sharing of electrons Ionic bond = Transfer of electrons Metallic bond = Sea of delocalized electrons Signup and view all the answers

Match the term with its implication:

Permanent dipole = Indicates polarity of molecules Asymmetrical charge distribution = Leads to dipole interactions Polar molecule = Has a dipole moment Nonpolar molecule = Does not produce a net dipole moment Signup and view all the answers

Match the bond with its electron affinity:

Cl-H bond = Cl attracts electrons more H-H bond = Electrons shared equally O-H bond = O draws electrons significantly C-C bond = Equal attraction in sigma bond Signup and view all the answers

Match the following elements with their role in hydrogen bonding:

Oxygen = Highly electronegative atom that can bond with hydrogen Hydrogen = Becomes δ+ charged when bonded to O, N or F Nitrogen = Another electronegative atom involved in hydrogen bonding Fluorine = The most electronegative element capable of hydrogen bonding Signup and view all the answers

Match the following properties of water with their causes:

High boiling point = Strong hydrogen bonding High surface tension = Intermolecular forces Higher density in liquid than solid = Hydrogen bond structure in ice Anomalous properties = Presence of hydrogen bonds Signup and view all the answers

Match the following types of intermolecular forces with their definitions:

Hydrogen bonds = Strong bonds between molecules with hydrogen and O, N or F Permanent dipole – permanent dipole = Interaction between polar molecules Dispersion forces = Induced dipole interactions due to electron movement Covalent bonds = Strong bonds within a molecule Signup and view all the answers

Match the following molecular scenarios with their characteristics:

Solid H2O = Hydrogen bonds maintain a fixed structure Liquid H2O = Molecules can move but are still held together by hydrogen bonds Ice = Lower density due to expanded hydrogen-bonded structure Steam = Higher energy state where hydrogen bonds are broken Signup and view all the answers

Match the following terms with their relevant scenarios in water's behavior:

Enthalpy of vaporization = Energy required to boil water Melting point = Energy needed to transition from solid to liquid Boiling point = Temperature at which water vaporizes Surface tension = Resistance of water to increase surface area Signup and view all the answers

Match the following elements with their common characteristics in hydrogen bonding:

O = Forms two hydrogen bonds N = Bonds with δ+ hydrogen F = Highly reactive due to electronegativity H = Participates in hydrogen bonding but not as an acceptor Signup and view all the answers

Match the following water behaviors with their implications:

High melting point = Comparison to other simple molecules High boiling point = Increased energy requirement due to hydrogen bonds High surface tension = Significant impact on water's interaction with other substances Anomalous properties = Unique behavior due to hydrogen bonding Signup and view all the answers

Match the following characteristics of hydrogen bonds with their significance:

Strong intermolecular forces = Explanation for unusual properties of water Bonding angles = Influence on molecular geometry Lone pairs = Necessary for forming hydrogen bonds Polarization of hydrogen = Allows for bond formation with electronegative atoms Signup and view all the answers

Match the following molecules with their related hydrogen bonding characteristics:

Water (H2O) = Can form two hydrogen bonds Ammonia (NH3) = Can form one hydrogen bond per molecule Hydrogen fluoride (HF) = Capable of very strong hydrogen bonds Methane (CH4) = Cannot form hydrogen bonds at all Signup and view all the answers

Study Notes