SCH3U7 - Topic 4: Bonding Review SL Which of these bonding types would not be classified as strong? Metallic Covalent Ionic Dipole dipole The bond dissociation energy of NaCl is 411 kj mol -1, while that of N2 is 945 kj mol -1. What conclusion can correctly be deduced from this information? Ionic bonding is stronger than covalent bonding. Covalent bonding does not involve electrostatic attraction between oppositely charged particles. More energy would be required to separate the ions in one mole of sodium chloride than to separate the atoms in one mole of nitrogen molecules. The triple covalent bond in nitrogen is stronger than the average ionic bond in sodium chloride. Which list below contains only ionic compounds? CaCO3, H2O, LiOH NH3, K2O, HNO3 LiOH, CaCO3, MgO NO2, MgO, CuCl2 Which of these statements about the formation of an ionic compound from a metal and a non-metal is true? I. Metal atoms donate electrons to the non-metal atoms. II. The non-metal atoms acquire a positive charge and the metal atoms a negative charge. III. Metal atoms form ions with smaller radii than their atomic radii. II and III only I and II only I, II and III I and III only Lithium has an atomic number of 3 and oxygen an atomic number of 8. What is the chemical formula of lithium oxide? Li2O
Li2O3 LiO LiO2 Element X has the electron configuration 2,8,3. Element Y has the configuration 2,8,6. What is the chemical formula of the compound formed between these two elements? X3Y2 XY XY3 X2Y3 Which of the following statements is correct in regard to ionic compounds? Like charged ions are as close together as possible. The ratio of positive to negative ions is always 1:1. Like charged ions are as far apart as possible. A state of maximum potential energy is achieved. What is the name of the compound with the chemical formula KHCO3? Potassium hydrogen carbide Phosphorous carbonate Potassium carbonate Potassium hydrogen carbonate Which list below contains only properties of metals? Good electrical conductivity; low boiling point; low density High melting point; high thermal conductivity; brittle Good electrical conductivity; lustrous; malleable Non-conductive; hard; malleable Which of the following statements best describes why solid metals are excellent electrical conductors? Metal cations are delocalized and so are free to move in all directions The valence electrons in metals are delocalized
Metal atoms are only loosely bonded to one another Metal cations are arranged in a three-dimensional network Which statement best describes metallic bonding? An array of metal atoms loosely bonded together. A network of positive ions and electrons held together by magnetic attractions. A network of positive and negative ions held together by electrostatic attractions. A network of positive ions with delocalized electrons moving through the network. Which statement best describes why metals are malleable? The cations can be moved relative to one another without destroying the bonding within the metal. The cations and anions can be moved relative to one another without destroying the bonding within the metal. The bonding in metals is very weak and so is easily disrupted. The delocalized electrons are able to move in response to an applied potential difference. Which list contains only molecular compounds? CH4, SO3, NH3, H2O H2O, CaO, F2, H2S LiOH, NaCl, MgO, CaCO3 H2O, Mg, CCl4, OCl2 How many electrons are involved in single, double and triple covalent bonds, respectively? 1, 2, 3 1, 3, 6 2, 3, 4 2, 4, 6 Only one of the following molecules exists. Which one is it? CCl3 HF2 HS
PH3 Which of the following molecules has the greatest number of non-bonding outer shell electron pairs? N2 H2S F2 NH3 Which statement is correct in regard to the molecule shown below? It will contain polar bonds and be polar. It will contain polar bonds but be non-polar. It will form a three-dimensional network solid. It will be non-polar and contain no polar bonds. What shape is the OCl2 molecule? Pyramidal Linear V-shaped Tetrahedral An atom of element X forms three single covalent bonds with atoms of element Y. The molecule, XY3, has no lone pairs in its structure. What would the bond angle XYX in this molecule be? 109 120 90 180 For which of the following species is the molecular shape incorrectly stated? H2O V-shaped SO2 linear NH4 + tetrahedral
PH3 pyramidal What is the name given to different structural forms of the same element? Allotropes Isotopes Alkaloids Isomers Which of the following properties applies to all three allotropes of carbon: diamond, graphite and buckyballs? I. High melting point II. Delocalized electrons present III. Covalently bound I, II and III II and III only I and III only I and II only Which of the following lists those forms of carbon that have hexagonal rings of covalently bonded carbon atoms in their structure? Nanotubes and buckyballs only Graphite, nanotubes and buckyballs only Diamond, graphite and nanotubes only Graphite and nanotubes only When fluorine forms a liquid, what type of intermolecular bonds are present? Covalent bonding Hydrogen bonding Van der Waals forces Dipole dipole bonds Which of the following molecules is expected to exhibit hydrogen bonding? HCl HF
CH4 H2S Methane (CH4) boils at approximately 130 C below the boiling point of ammonia (NH3). How is this difference in boiling points best explained? The presence of hydrogen bonding in ammonia. The stronger covalent bonds in ammonia. The ionic bonds in ammonia. The stronger van der Waals forces in ammonia. Which of the following lists the substances in order of increasing melting points? CH4, H2S, BaO, SiO2 CH4, H2S, SiO2, BaO SiO2, BaO, H2S, CH4 H2S, BaO, SiO2, CH4 X is a brittle substance with a very high melting point. As a solid, X does not conduct electricity, but it conducts when molten. Which of the listed properties shows that X is not a covalent network lattice? Conductivity when molten Brittleness Non-conductive in the solid state High melting point Which statement regarding ionic compounds is true? They do not conduct electricity under any circumstances. They conduct electricity when in the liquid state. They conduct electricity in both the liquid and the solid states. They conduct electricity only in the solid state. Why is sodium iodide (NaI) a non-conductor of electricity at room temperature? It consists of uncharged molecules. It has strong covalent bonds which prevent electrons from moving.
It does not contain ions or mobile electrons. It contains ions which are not mobile. SCH3U7 - Topic 4: Bonding HL Review When one s orbital and three p orbitals form four orbitals of equal energy, the result is... one hybrid sp 3 orbital. four sp 3 hybrid orbitals. four hybrid d 4 orbitals are created. a molecule that does not exist. During hybridization of orbitals, the number of hybrid orbitals produced is equal to... the total number of energy levels that each atom has. the total number of electrons involved in the bond. the number of valence electrons. the number of orbitals that have combined. Which one of the following atoms does not obey the octet rule in the compound given? Nitrogen in NH3 Fluorine in BF3 Sulfur in SF6 Carbon in CO2 Which molecule exhibits resonance? CO3 2- CO2 BF3 BeI2 Resonance refers to... bonding in molecules or ions in which the particles vibrate. bonding of unstable isotopes.
bonding that occurs in a molecule of O2. bonding in molecules or ions that cannot be correctly represented by a single Lewis structure. What is the best description of the nitrogen-oxygen bond lengths in NO3 -? One long and two short bond lengths. Three bonds of different lengths. One short and two long bond lengths. Three bonds of the same length. State the number of sigma and pi bonds in the molecule and the hybridization of the carbon atom in the molecule below? 3 sigma, 1 pi, sp 2 4 sigma, 1 pi, sp 3 3 sigma, 2 pi, sp 3 4 sigma, 1 pi, sp 2 Which of the following contains a bond angle of 90? I. PC14 + II. PCl5 III. PCl6 - II and III only I and II only I, II and III I and III only Which statement about σ and π bonds is correct? σ bonds are formed by either s or p orbitals, π bonds are formed only by p orbitals. σ bonds are formed only by s orbitals and π bonds are formed only by p orbitals. σ and π bonds are formed by either s or p orbitals. σ bonds are formed only by p orbitals and π bonds are formed only by s orbitals. How many resonance structures can exist for BF3?
2 3 1 4 Upon hybridization of one s and one p orbital there exists... four orbitals in a tetrahedral configuration. two orbitals at 180. three orbitals in a plane. two mutually perpendicular π orbitals. Consider the following statements. I. All carbon-oxygen bond lengths are equal in CO3 2-. II. ll carbon-oxygen bond lengths are equal in CH3COOH. III. All carbon-oxygen bond lengths are equal in CH3COO -. Which statements are correct? II and III only I and III I and II only. I, II and III Which of the following correctly describes a π bond? It is formed by the interaction of p-orbitals and has a high electron density on the internuclear axis. It is formed by the interaction of the p-orbitals and has a low electron density on the internuclear axis. It is formed by the interaction of the s-orbitals and has a low electron density along the internuclear axis. It is formed by the interaction of the s-orbitals and has a high electron density along the internuclear axis. How many π bonds are there in CO2? 2 1 4 3
What is the shape of a XeF4 molecule? Square planar Octahedral Tetrahedral Trigonal bipyramidal The bond angles in an octahedral shaped molecule are... only 109.5. both 90 and 120. only 90. only 120. What type of hybridization occurs in the nitrogen atom for bonding in a NH3? sp 2 sp sp 3 sp 3 d What is the total number of π bonds in a molecule of benzene when drawn as resonance structures? 1 3 2 6 In which of the following molecules would delocalized electrons be found in π bonds? I. C6H6 II. CO3 2- III. CH3COOH I, II and III I only I and II III only
In the nitrite ion, NO2 -... both bonds are single bonds. both bonds are the same length. There are two double bonds. one bond is double and one bond is single. State the shape of an ICl3 molecule and the size of the bond angles which are present in the molecule? Tetrahedral 104.5 T-shaped 90 and 180 Trigonal pyramidal 107 Trigonal planar 120 State the hybridization and the shape around each of the two nitrogen atoms in the diazene, N2H2, molecule? sp 3 and trigonal pyramidal. sp 2 and trigonal planar. sp 2 and bent linear sp 3 and trigonal planar. State the hybridization and molecular geometry for CH4? sp 3 and tetrahedral. sp 3 and trigonal pyramidal. sp 2 and trigonal planar. sp 2 and tetrahedral The features which should be included in a correct description of the bonding in a molecule of benzene are... I. delocalized electrons and π bonds II. double bonds between carbon atoms III. sp 2 hybridization of carbon atoms. I and III I, II and III I only II and III
Double bonds are formed by σ and π bonds. Triple bonds are formed by σ and π bonds. one, two, one, two one, one, one, one one, one, one, two one, one, two, two