CHEM 1315 EXAM 2 REVIEW
What is the correct formula for ammonium sulfide? (NH4)2S (NH4)2SO4 NH4SO4 NH4S NH3SO4
(NH4)2S The sulfide ion is S2-, so (NH4)2S is correct.
Which of the following molecules are polar (will have a net dipole moment)? 1. H2O 2. CO2 3. CIF3 4. PCl5 5. BF3 1, 2, and 3 1 and 3 2, 4, and 5 3 only All of these are polar
1 and 3 **Draw it out**
Identify the molecules below that obey the octet rule: 1. CO32 - 2. BH3 3. I3- 4. GeF4 1 and 2 1 and 4 2 and 4 1, 2, and 4 4 only
1 and 4 **Draw it out**
A 1.2 x 10^7 μg sample of Cr2(SO4)3 contains how many sulfur atoms?
1.2 x 10^7 μg x (1g/10^6μg) x (1mol Cr2(SO4)3/392.21g Cr2(SO4)3) x (3molS/1mol Cr2(SO4)3) x (6.022x10^23 atoms S/1molS) = 5.52x10^22 atoms S
The mass (in grams) of carbon in 112 grams of acetylsalicylic acid (aspirin), C9H8O4, is:
112g C9H8O4 x (1mol C9H8O4/180.154g C9H8O4) x (9mol C/1mol C9H8O4) x (12.011g C/1mol C) = 67.2g C
How many lone pairs of electrons are on the Xe atom in XeF4?
2 **Draw it out**
Which of the following pairs of formulas and names are correct? 1. S2Cl2, sulfur dichloride 2. XeO4, xenon tetroxide 3. HClO2, chlorous acid 4. HNO2, nitric acid 5. Fe2O3, iron (II) oxide 1 and 2 1 and 5 2 and 3 3, 4, and 5 4 and 5
2 and 3 S2Cl2 is disulfur dichloride HNO2 is nitrous acid Fe2O3 is iron (III) oxide
An ionic compound has the formula M2(CO3)3. What is the possible identity of the ion M? 1. iron (II) 2. iron (III) 3. Cu (I) 4. Cu (II) 5. Al3+ 2 and 5 2 and 4 3 and 4 1 and 4 1 and 5
2 and 5 Carbonate has a -2 charge, and there are three carbonate polyatomic ions present. To balance out this -6 charge (3 times -2), the metal ion would have to contribute an overall + 6 charge. This can only be achieved with 2 (the number of metal ions that we have) times +3. The metal ion would have to have a +3 charge. In this group, only Iron (III) and Al3+ have this charge.
Given hypothetical metals represented by M in the formulas below, which of the following assignments of M's identity are not possible? 1. MSO4 M = Ca 2. M(NO3)2 M = K 3. M2S M = Cu (I) 4. M2O3 M = Al 5. M2 CO3 M = Zn 1 and 2 3 and 4 4 and 5 1 and 5 2 and 5
2 and 5 The nitrate ion has a -1 charge, and the formula indicates that the ionic compound has two nitrate ions. With only one metal ion in the formula, the metal would have to achieve a +2 charge state. Potassium forms a +1, so this is incorrect. The carbonate ion has a -2 charge. To balance this -2 charge, the two metal ions in the formula would have to have a +1 charge. Zinc always forms a +2 ion, so this is not possible.
Which of the following incorrectly identifies a possible metal ion based on the corresponding formula indicated? 1. MSO4, M = Ba 2. M(NO3)2, M = Ag 3. M2S, M = Na 4. M2O3, M = Al 5. MCO3, M = K 1 and 3 2 and 5 3 and 4 1, 2 and 5 2, 4 and 5
2 and 5 The nitrate ion has a -1 charge, and the formula indicates that the ionic compound has two nitrate ions. With only one metal ion in the formula, the metal would have to achieve a +2 charge state. Silver only forms a +1 ion, so this is incorrect. The carbonate ion has a -2 charge. To balance this -2 charge, the one metal ion in the formula would have to have a +2 charge. Potassium always forms a +1 ion, so this is not possible.
The best Lewis structure for SOCl2, where S violates the octet rule, will have [x] single bond(s), [y] double bond(s), and [z] lone pair(s) around the central atom. The electron domain geometry around the central S atom is [e].
2 single 1 double 1 lone pair(s) tetrahedral
The best Lewis structure for the SeO32- ion will have [x] single bond(s), [y] double bond(s), and [z] lone pair(s) around the central atom. The electron domain geometry around the central atom is [e].
2 single 1 double 1 lone pair(s) tetrahedral
Nutrasweet is an artificial sweetener with the molecular formula C14H18N2O5. Calculate the number of nitrogen atoms present in 250. mg of Nutrasweet.
2.50mg x (1g/1000mg) x (1mol C14H18N2O5/294.30g C14H18N2O5) x (2molN/1mol C14H18N2O5) x (6.022x10^23 atomsN/1molN) = 1.02x10^21 atoms N
How many lone pairs are on Br in BrF2—? 0 1 2 3 4
3 **Draw it out**
Which of the following combinations of names and formulas are correct? 1. HNO3: nitrous acid 2. Cl2O7: chlorine heptoxide 3. HCl: hydrochloric acid 4. S2F4: disulfur tetrafluoride 5. ClF: monochlorine monofluoride 1, 2, and 4 2, 4, and 5 3 and 5 3 and 4 4 and 5
3 and 4 1. HNO3: nitric acid 2. Cl2O7: dichlorine heptoxide 3. HCl: hydrochloric acid 4. S2F4: disulfur tetrafluoride 5. ClF: chlorine monofluoride
Which of the following formulas correctly corresponds to the name given? 1. sodium nitride: NaNO3 2. magnesium hypochlorite: Mg(ClO2)2 3. calcium phosphate: Ca3(PO4)2 4. lead (IV) bromide: Pb4Br 5. aluminum hydroxide: Al(OH)3 1, 2, and 5 1, 3, and 4 2, 3, and 4 1 and 3 3 and 5
3 and 5 Sodium nitride is Na3N Magnesium hypochlorite is Mg(ClO)2 Lead (IV) bromide is PbBr4
Calculate the number of hydrogen atoms present in 39.6 grams of (NH4)2SO4.
39.6g (NH4)2SO4 x (1mol (NH4)2SO4/132.15g (NH4)2SO4) x (8molH/1mol (NH4)2SO4) x (6.022x10^23 atomsH/1molH) = 1.44x10^24 atoms
Which of the following formulas correctly correspond to the names given? 1. potassium carbonate: PCO3 2. zinc chloride: ZnCl 3. magnesium phosphide: Mg3(PO4)2 4. ammonium nitrate: NH4NO3 5. sodium chlorate: NaClO3 2, 3, and 4 3 and 5 1, 2, and 4 3, 4, and 5 4 and 5
4 and 5 Potassium carbonate is K2CO3 Zinc chloride is ZnCl2 Magnesium phosphide is Mg3P2
A molecule, that is sp3d2 hybridized and has a molecular geometry of square planar, has ________ bonding groups and ________ lone pairs around its central atom. 2, 3 3, 2 4, 1 4, 2 5, 1
4, 2 square planar AB4E2
Which ionic compound would be expected to have the highest lattice energy? Na2O, MgO, Al2O3, CO2
Al2O3 For this question, we can disregard CO2 because it is not an ionic compound. Lattice Energy is impacted by two main factors: Ion size & Ion charge. For the three ionic compounds, oxygen is in common, but note the charges of the metal ions are different. These three metal ions will be of a similar size, so we can rank these relatively by the charge of the ions. The Al3+ charge will have the strongest electrostatic attraction to the oxide ion. A lattice energy table is not needed to answer this question.
Which ionic compound would be expected to have the highest lattice energy? NaCl ,MgO, AlF3, Al2O3
Al2O3 Lattice Energy is impacted by two main factors: Ion size & Ion charge. For this question, we look to the charge since the metal ions are of a similar size. The greater the charges in an ionic compound, the higher the lattice energy. The sodium +1 ion/chloride -1 ion will have a lower lattice energy compared to the magnesium +2 ion/oxide -2 ion. The aluminum +3 ion/fluoride -1 ion will be greater than MgO, and then a comparison of the two aluminum ion compounds shows the higher charge with the aluminum ion +3 and the oxide ion -2. A lattice energy table is not needed to answer this question.
Consider the following electron configurations for neutral atoms: I= 1s2 2s2 2p6 3s2 II= 1s2 2s2 2p6 3s2 3p4 III= 1s2 2s2 2p6 3s2 3p6 Which atom would be expected to have the largest third ionization energy? atom I atom II atom III All of these atoms would be expected to have the same third ionization energy.
Atom I IE3: The loss of three electrons from the atom. A large increase in ionization energy would indicate that the atom lost all of its valence electrons plus one of the core electrons. For this group, only atom I has two electrons in the valence. The removal of a third electron (IE3) would show a large jump in the amount of energy required. Atom 1's electron configuration indicates that this is Mg (this information isn't needed to answer the question, but might help our more visual learners zero in on the periodic table for a better visual clue of electron configuration.
Which alkaline earth metal reacts the most vigorously with water at room temperature? Be, Ca, Ba, Sr
Ba The larger the atom, the farther away from the nucleus the valence electrons will be - this results in the electrons being lost more easily down a group/family. Due to distance and shielding, the electrons that are further and further away from the nucleus "feel" the attraction to the electrons in the nucleus to a lesser degree.
Group 2A metals tend to be somewhat less reactive than alkali metals, and the order of their reactivity is: Ba > Sr > Ca > Mg > Be Be > Mg > Ca > Sr > Ba Ca > Mg > Be > Ba > Sr Sr > Ca > Mg > Be > Ba
Ba > Sr > Ca > Mg > Be The larger the atom, the farther away from the nucleus the valence electrons will be - this results in the electrons being lost more easily down a group/family. Due to distance and shielding, the electrons that are further and further away from the nucleus "feel" the attraction to the electrons in the nucleus to a lesser degree.
Which of the following molecular geometries will ALWAYS be polar? Linear Trigonal Planar Bent Tetrahedral Trigonal pyramidal
Bent Trigonal pyramidal
As the number of bonds between two carbon atoms increases, which of the following decreases? Bond length Bond strength Both bond length and bond strength Neither bond length nor bond strength
Bond length Single bonds are longer than double bonds between atoms, and double bonds are longer than triple bonds. For Carbon bonding with another Carbon, this means that the order of bond length looks like this: C - C > C = C > C ≡ C
Which of the following requires that resonance structures be drawn to accurately represent possible Lewis structure(s)? CH3OH BF3 CH4 SF6 CHO2-
CHO2- ***Draw them out***
Which formula/name combination below is incorrect? K3PO4: potassium phosphate H2SO3: Sulfurous acid CaS: calcium sulfate NH4NO2: ammonium nitrite HBrO3: bromic acid
CaS: calcium sulfate This is calcium sulfide, not sulfate.
The ionization energies for an element were reported as shown below. The element represented by these ionization energies is _____________. IE1 = 1,086 kJ/mol IE2 = 2,353 kJ/mol IE3 = 4,621 kJ/mol IE4 = 6,223 kJ/mol IE5 = 37,831 kJ/mol Be B C Li He
Carbon IE5: The loss of five electrons from the atom shows a very large increase in ionization energy. This increase reflects the atom having lost all of its valence electrons, then removing one of the core electrons. Therefore, the element must have four valence electrons. Carbon is the only element in this group that has four electrons in its valence shell.
When hydrogen is added to the carbonate ion, what is the name of the acid formed? Carbonate acid Sulfuric acid Carbonous acid Carbonic acid Carbon acid
Carbonic Acid Carbonic acid is H2CO3
Arrange the following elements in order of increasing atomic radii: K, Na, Mg, Cs, Cl. Na < Mg < Cl < K < Cs Cl < Mg < Na< K <Cs Cs < K < Cl < Mg < Na Cl < Mg < Cs < K <Na Cl < Mg < Na< Cs <K
Cl < Mg < Na< K <Cs The size of a neutral atom increases down a group/family on the periodic table (larger n, more shells) and decreases across the period (increasing effective nuclear charge).
Which of the following statements are false? I. The first ionization energy of sulfur is larger than that of phosphorus. II. The second ionization energy of potassium is larger than the second ionization energy of calcium. III. The effective nuclear charge increases across a period. IV. Anions will be smaller than their parent atom because of the repulsion of the electrons of the ion. I, II, and IV III and IV II, III, and IV I and III I and IV
I and IV Ionization Energy decreases slightly between three electrons in the p orbitals (P) and four electrons in the p orbitals (S), due to the higher energy status (repulsion) of having two electrons in one of the p orbitals and two unpaired (S) as compared to one electron in each p orbital (P). Anions are always larger than their parent atom. The proton number of the neutral atom and the ion are the same. Increased electron(s) with the same proton number results in increased repulsions, and a slightly larger ion size.
Which of the following statement(s) about IBr5 is/are true? I. The Br-I-Br bond angle is less than 90o, the hybridization is sp3d2, and molecule is polar. II. The molecule has an octahedral electron geometry, and it contains a lone electron pair. III. The molecule has a square planar molecular geometry, and it is nonpolar. IV. Every atom in the molecule has a formal charge of 0. I II I and III I, II, and III I, II, and IV
I, II, IV **Draw it out**
Which of the following pairs of names and formulas are not correct? I. tetraphosphorus decasulfide P4S10 II. iron (II) nitrate Fe(NO3)3 III. magnesium phosphide Mg3(PO4)2 IV. potassium chlorate KClO3 II and III III and IV I, II, and III II, III, and IV I, III and IV
II and III S2Cl2 is disulfur dichloride HNO2 is nitrous acid Fe2O3 is iron (III) oxide
Which of the following molecules are polar? I. PF6- II. NCl3 III. XeF4 IV. IF5 V. BF3 I, II, and III I, II, and IV II and IV II, III, and IV II, IV, and V
II and IV
In which of the following molecules does the central atom not obey the octet (or duet) rule? I. CO2 II. BrF3 III. XeF2 IV. NH4+ V. SF4 I, II, and III I, III, and IV II, III, and V II, III, IV, and V All of these molecules violate the octet rule
II, III, and V **Draw them out**
Which of the following statements is correct? I. In structures where resonance occurs, the bond lengths fluctuate rapidly. II. In structures where resonance occurs, the bond strengths vary with time. III. In structures where resonance occurs, the electrons are delocalized. I only II only III only I and II I and III
III only Electrons move so rapidly that individual single and/or double bonds cannot be measured. Instead, bond lengths stay a hybrid of the two bond types - they will be longer than a double bond, and shorter than a single bond would be without resonance. Bond strength will not vary, either.
The three spheres below represent K+, Ca2+, and Cl-, not necessarily in that order. A, r= 100 pm B, r=138 pm C, r=184 pm Which sphere most likely represents the K+ ion? Which sphere most likely represents the Ca2+ ion? Which sphere most likely represents the Cl⁻ ion?
K+=B Ca2+=A Cl-=C These ions are isoelectronic (all the ions have the same number of electrons). The ion with the MOST protons will be the smallest and the ion with the LEAST protons will be the biggest. The larger number of protons in a group with the same number of electrons will have the greatest attraction ("pull" on the electrons) to the nucleus.
Calcium reacts with a certain element to form a compound with the general formula CaX. What would the most likely formula be for the compound formed between potassium and element X? K2X KX2 K2X3 K2X2 KX
K2X The calcium ion has a +2 charge, and the formula indicates that the ionic compound has one calcium ion. With only one X anion in the formula, the anion would have a -2 charge. Potassium always forms a +1 ion. To balance the -2 charge of the anion, X, two potassium ions are needed.
Which ionic compound would be expected to have the highest lattice energy? Li2O, Na2O, K2O, Rb2O
Li2O Lattice Energy is impacted by two main factors: Ion size & Ion charge. For this question, the oxide ion is common to all choices. Only the alkali metal ion changes. The smaller the ion (Li+), the greater the lattice energy. A lattice energy table is not needed to answer this question.
Which of the following ionic compounds would be expected to have the highest lattice energy? LiCl, NaCl, KCl, RbCl
LiCl Lattice Energy is impacted by two main factors: Ion size & Ion charge. For this question, the chloride ion is common to all choices. Only the alkali metal ion changes. The smaller the ion (Li+), the greater the lattice energy. A lattice energy table is not needed to answer this question.
An element M reacts with chlorine to form MCl2, with oxygen to form MO, and with nitrogen to form M3N2. The most likely candidate for the element is Li Mg Al Si
Mg The chloride ion has a -1 charge, and there are two chloride ions present. To balance out this -2 charge (2 times -1), the metal ion would have to contribute an overall + 2 charge. This can only be achieved with 1 (the number of metal ions that we have) times +2. The metal ion would therefore have a +2 charge. In this group, only Mg forms a +2 ion.
Arrange the ions N3-, O2-, Mg2+, Na+, and F- in order of increasing ionic radius, starting with the smallest first. Mg2+, Na+, F-, O2-, N3- N3-, Mg2+, O2-, Na+, F- N3-, O2-, Mg2+, F-, Na+ N3-, O2-, F-, Na+, Mg2+
Mg2+, Na+, F-, O2-, N3- In an isoelectronic series, where all the ions have the same number of electrons, the ion with the MOST protons will be the smallest and the ion with the LEAST protons will be the biggest. The larger number of protons in a group with the same number of electrons will have the greatest attraction ("pull" on the electrons) to the nucleus.
The four spheres below represent Na+, Mg2+, F⁻, and O2-, not necessarily in that order. A, r=72 pm B, r=102 pm C, r=133 pm D, r=140 pm Which sphere most likely represents the Mg2+ ion? Which sphere most likely represents the F- ion? Which sphere most likely represents the O2- ion? Which sphere most likely represents the Na+ ion?
Mg2+= A F-= C O2-= D Na+= B These ions are isoelectronic (all the ions have the same number of electrons). The ion with the MOST protons will be the smallest and the ion with the LEAST protons will be the biggest. The larger number of protons in a group with the same number of electrons will have the greatest attraction ("pull" on the electrons) to the nucleus.
Which of the following correctly lists these atoms in order of decreasing electronegativity: K, P, N, Cs, Ga? N > P > Ga > K > Cs N > Ga > P > K > Cs N > Ga > P > Cs > K N > K > P > Ga > Cs N > P > Cs> Ga > K
N > P > Ga > K > Cs Use the electronegativity trend and the periodic table as a visual tool: electronegativity increases up a group/family and across a period.
Which of these molecules has resonance structures? HCN BrF5 COCl2 N3— BH3
N3- ***Draw it out***
Which process below is associated with the lattice energy for sodium chloride? NaCl(s) → Na+(g) + Cl-(g) NaCl(g) → Na+(g) + Cl-(g) Na(s) + 1/2 Cl2(g) → NaCl(s) NaCl(s) + H2O(l) → Na+(aq) + Cl-(aq)
NaCl(s) → Na+(g) + Cl-(g) Lattice Energy is defined by the amount of energy required to disrupt one mole of a solid ionic compound to form ions in the gaseous state. Only the choice (below) indicates the correct states (s or g) for the representation of the reaction. NaCl(s) → Na+(g) + Cl-(g)
Which of the following ionic compounds would be expected to have the highest lattice energy? NaF, NaCl, NaBr, NaI
NaF Lattice Energy is impacted by two main factors: Ion size & Ion charge. For this question, sodium ion is common to all choices. Only the halogen ion changes. The smaller the ion (F-), the greater the lattice energy. A lattice energy table is not needed to answer this question.
Which of one of the following statements is false? The effective nuclear charge increases across a period. Metallic character increases down the alkali metal group on the periodic table. The atomic radius of neutral atoms decreases across a period. Ionization energy decreases down a group or family on the periodic table. Nitrogen has a lower ionization energy than Oxygen.
Nitrogen has a lower ionization energy than Oxygen. Ionization Energy increase up a family/group on the periodic table (electrons are closer to the nucleus and therefore harder to remove) and increases across a period (increased effective nuclear charge). However, watch out for the two discontinuities that impact ionization energies: 1. slight decrease from 2 electrons in the s to 1 in the p orbitals between the s block and p block 2. slight decrease in IE between three electrons in the p orbitals and four electrons in the p orbitals.
Which ionization process requires the most energy? P(g) → P+(g) + e- P+(g) → P2+(g) + e- P2+(g) → P3+(g) + e- P3+(g) → P4+(g) + e-
P3+(g) → P4+(g) + e- Each subsequent removal of an electron will be increasingly more difficult, resulting in higher ionization energies for IE2, IE3, IE4, etc. compared to IE1.
When a fluorine atom bonds with a chlorine atom, the bond that forms between them is best described as _________. Nonpolar covalent Ionic-covalent Ionic Polar covalent
Polar Covalent Both fluorine and chlorine are nonmetals, so this will be a covalent bond. Since the electronegativities of these two elements differ, we would classify this as a polar covalent bond.
Which of the following does not have the ions arranged correctly in order of increasing ionic radius? Mg2+ < Ca2+ < Sr2+ Al3+ < Mg2+ < Na+ F - < Cl - < Br - F - < Se2- < Cs+ Rb+ < Sr2+ < In3+
Rb+ < Sr2+ < In3+ In an isoelectronic series, where all the ions have the same number of electrons, the ion with the MOST protons will be the smallest and the ion with the LEAST protons will be the biggest. The larger number of protons in a group with the same number of electrons will have the greatest attraction ("pull" on the electrons) to the nucleus.
When bonding with a chlorine atom, which of the following atoms will yield the least polar bond? I S P Ca Se
S Both iodine and chlorine are nonmetals, so this will be a covalent bond. Since the electronegativities of these two elements differ, we would classify this as a polar covalent bond. A quick check of the electronegativity trend using the periodic table as a visual tool shows us that Chlorine is more electronegative than Iodine, so it will draw the electron density towards itself in the shared pair of electrons. A check of the proximity of the elements on the periodic table will often be sufficient to determine the relative polarity of the bond. The closer the elements are to one another, the more similar the electronegativity values and the less polar the bond. The farther apart the elements are, the more polar the bond (even to the point of being ionic).
The equation below represents the ___ionization energy of Phosphorus. P+(g) → P2+(g) + e-
Second IE2: The loss of a second electron. The equation must start with the +1 ion since one electron has already been removed.
Of the following, which element has the highest first ionization energy? Aluminum Magnesium Silicon Sodium
Silicon Ionization Energy increase up a family/group on the periodic table (electrons are closer to the nucleus and therefore harder to remove) and increases across a period (increased effective nuclear charge). However, watch out for the two discontinuities that impact ionization energies: 1. (slight decrease from 2 electrons in the s to 1 in the p orbitals between the s block and p block 2. slight decrease in IE between three electrons in the p orbitals and four electrons in the p orbitals.
Which of one of the following statements is false? Strontium is more reactive than calcium. Cesium is more reactive than sodium. Sodium is less reactive than magnesium. Potassium is more reactive than calcium. Calcium is more reactive than magnesium.
Sodium is less reactive than magnesium. The larger the atom, the farther away from the nucleus the valence electrons will be - this results in the electrons being lost more easily down a group/family. Due to distance and shielding, the electrons that are further and further away from the nucleus "feel" the attraction to the electrons in the nucleus to a lesser degree.
Which of the following molecular geometries will ALWAYS be polar? Octahedral Square Planar Square Pyramidal See-Saw T-Shaped
Square Pyramidal See-Saw T-Shaped
The equation below represents the ___ ionization energy of Oxygen. O2+(g) → O3+(g) + e-
Third IE3: The loss of a third electron. The equation must start with the +2 ion since two electrons have already been removed.
What type of molecular geometry can occur with sp3 hybridization? Trigonal planar T-shaped Square planar Trigonal pyramidal Trigonal bipyramidal
Trigonal pyramidal sp3: 4 electron domains
Arrange in order from the smallest to the largest bond angle: CH3+, NF3, NH4+, XeF4. CH3+, NF3, NH4+, XeF4 NF3, NH4+, XeF4, CH3+ XeF4, NH4+, NF3, CH3+ XeF4, NF3, NH4+, CH3+
XeF4, NF3, NH4+, CH3+ CH3+: trig. planar= ~120 NF3: trig. pyramidal= ~107 NH4+: Tetrahedral= ~109.5 XeF4: square planar= ~90
The hypothetical element Xium (X) has an atomic mass of [M] g/mol. If the formula for Xium phosphate is X3(PO4)2, the molar mass of xium phosphate is _____ g/mol. Report the formula/steps to solve this.
[M] will vary by question Calculate molar mass: (3x[M]g/mol) + (30.974g/mol x2) + (15.999g/mol x8)= Molar Mass
The molecule XeF4 ___ the octet rule because _____.
[violates] [there are more than eight electrons around the central atom Xe].
The molecule NO2 ____ the octet rule because_____.
[violates] [there is an odd number of electrons so nitrogen cannot achieve an octet].
Vincristine, marketed as Oncovin, is a chemotherapeutic agent with a formula of C46H56N4O10 (molar mass = 824.96 g/mol). A [x] mg sample of Vincristine contains a mass of ___________ mg of oxygen. Report the formula/steps to solve this
[x] will vary [x]mg x (1g/1000mg) x (1mol C46H56N4O10/824.96g) x (10mol O/1mol C46H56N4O10) x (15.999gO/1mole O) x (1000mg/1g) = ______mg O
Vincristine, marketed as Oncovin, is a chemotherapeutic agent with a formula of C46H56N4O10 (molar mass = 824.96 g/mol). A [x] mg sample of Vincristine contains a mass of ___________ mg of carbon. Report the formula/steps to solve this
[x] will vary [x]mg x (1g/1000mg) x (1mol C46H56N4O10/824.96g) x (46mol C/1mol C46H56N4O10) x (12.011gC/1mole C) x (1000mg/1g) = ______mg C
Vincristine, marketed as Oncovin, is a chemotherapeutic agent with a formula of C46H56N4O10 (molar mass = 824.96 g/mol). A [x] mg sample of Vincristine contains a mass of ___________ mg of nitrogen. Report the formula/steps to solve this
[x] will vary [x]mg x (1g/1000mg) x (1mol C46H56N4O10/824.96g) x (4mol N/1mol C46H56N4O10) x (14.007gN/1mole N) x (1000mg/1g) = ______mg N
Vincristine, marketed as Oncovin, is a chemotherapeutic agent with a formula of C46H56N4O10 (molar mass = 824.96 g/mol). A [x] mg sample of Vincristine contains a mass of ___________ mg of hydrogen. Report the formula/steps to solve this
[x] will vary [x]mg x (1g/1000mg) x (1mol C46H56N4O10/824.96g) x (56molH/1mol C46H56N4O10) x (1.008gH/1mole H) x (1000mg/1g) = ______mg H
Carmustine is a chemotherapeutic agent with a formula of C5H9Cl2N3O2 (molar mass = 214.05 g/mol). What mass (in grams) of Carmustine contains [x] x 10^22 carbon atoms? Report the formula/steps to solve this
[x] will vary by question [x] x 10^22 atoms C x (1mol C/(6.022x10^23atoms C) x (1mol C5H9Cl2N3O2/5mol C) x (214.05g/1mol)= _____g
Carmustine is a chemotherapeutic agent with a formula of C5H9Cl2N3O2 (molar mass = 214.05 g/mol). What mass (in grams) of Carmustine contains [x] x 10^22 chlorine atoms? Report the formula/steps to solve this
[x] will vary by question [x] x 10^22 atoms Cl x (1mol Cl/(6.022x10^23atoms Cl) x (1mol C5H9Cl2N3O2/2mol Cl) x (214.05g/1mol)= _____g
Carmustine is a chemotherapeutic agent with a formula of C5H9Cl2N3O2 (molar mass = 214.05 g/mol). What mass (in grams) of Carmustine contains [x] x 10^22 hydrogen atoms? Report the formula/steps to solve this
[x] will vary by question [x] x 10^22 atoms H x (1mol H/(6.022x10^23atoms H) x (1mol C5H9Cl2N3O2/9mol H) x (214.05g/1mol)= _____g
Carmustine is a chemotherapeutic agent with a formula of C5H9Cl2N3O2 (molar mass = 214.05 g/mol). What mass (in grams) of Carmustine contains [x] x 1022 nitrogen atoms? Report the formula/steps to solve this
[x] will vary by question [x] x 10^22 atoms N x (1mol N/(6.022x10^23atoms N) x (1mol C5H9Cl2N3O2/3mol N) x (214.05g/1mol)= _____g
Carmustine is a chemotherapeutic agent with a formula of C5H9Cl2N3O2 (molar mass = 214.05 g/mol). What mass (in grams) of Carmustine contains [x] x 1022 oxygen atoms? Report the formula/steps to solve this
[x] will vary by question [x] x 10^22 atoms O x (1mol O/(6.022x10^23atoms O) x (1mol C5H9Cl2N3O2/2mol O) x (214.05g/1mol)= _____g
ICl contains _______________. an ionic bond a nonpolar covalent bond a polar covalent bond, with a partial negative charge on the Cl atom a polar covalent bond, with partial negative charge on the I atom
a polar covalent bond, with a partial negative charge on the Cl atom Both iodine and chlorine are nonmetals, so this will be a covalent bond. Since the electronegativities of these two elements differ, we would classify this as a polar covalent bond. A quick check of the electronegative trend using the period table as a visual tool shows us that Chlorine is more electronegative than iodine, so will draw the electron density towards itself in the shared pair of electrons.
Which one of the following combinations of names and formulas is NOT correct? carbonic acid, H2CO3 potassium chlorate, KClO3 nitrous acid, HNO2 copper (II) chloride, CuCl2 calcium nitride, Ca(NO3)2
calcium nitride, Ca(NO3)2 calcium nitride is Ca3N2
When representing the difference in electronegativity between a sulfur atom and a chlorine atom in a bond, an arrow should be drawn over the bond pointing to ________, the _________ electronegative atom. sulfur, more sulfur, less chlorine, more chlorine, less
chlorine, more Use the electronegativity trend and the periodic table as a visual tool: electronegativity increases up a group/family and across a period. Chlorine is more electronegative, so will pull the electron density of the bond to itself, giving it the partial negative charge. Convention dictates that we draw an arrow over the bond, pointing to the more electronegative atom.
Compound A is a solid with a melting point of 825°C, and compound B is a gas at 25°C and one atmosphere pressure. Based on these data, one would expect compound A to be ionic and compound B to be covalent. compound A to be covalent and compound B to be ionic. both compounds to be covalent. both compounds to be ionic.
compound A to be ionic and compound B to be covalent. Ionic compounds have high melting and boiling pts. Generally, Covalent compounds will be in the gaseous state or possibly brittle or powdery solids at room temperature/pressure.
When electrons in a molecule move throughout the molecule, forming equivalent structures, the electrons are said to be______. ionic bonding. covalent bonding. polar covalent bonding. delocalized. a dipole moment.
delocalized.
The greater the electronegativity difference between two bonded atoms, the greater the bond order. greater the covalent character of the bond. greater the ionic character of the bond. more unstable the bond.
greater the ionic character of the bond. Think of bonding on a continuum: the more similar the electronegativities between atoms bonding, the less polar the bond (less ionic, more nonpolar covalent). The farther apart the atoms are on the periodic table, the greater the difference in electronegativity (an atom's ability to pull the electron density in a bond toward itself). The continuum goes from nonpolar covalent to polar covalent to ionic. The least polar bond is a nonpolar covalent and the most polar (to the point of electron transfer) is ionic. Polar covalent falls in between these extremes.
In general, at room temperature _____________________. ionic compounds are all solids and covalent compounds are all gases. ionic compounds are all solids, but covalent compounds may be solids, liquids, or gases. ionic compounds are all solids, and covalent compounds are liquids or gases. covalent compounds are all gases, but ionic compounds may be solids, liquids, or gases.
ionic compounds are all solids, but covalent compounds may be solids, liquids, or gases. Ionic compounds have high melting and boiling pts. Generally, Covalent compounds will be in the gaseous state or possibly brittle or powdery solids at room temperature/pressure.
Which of the following best describes ICl2-? It has a molecular geometry that is linear molecular shape with no lone pairs on the I atom. linear molecular shape with lone pairs on the I atom. non-linear molecular shape with no lone pairs on the I atom. non-linear molecular shape with lone pairs on the I atom.
linear molecular shape with lone pairs on the I atom. **Draw it out**
The correct name for Mn(CH3COO)4 is manganese(IV) acetate manganese(II) acetate manganese(1V) carbonate manganese(II) carbonate
manganese(IV) acetate The acetate ion can be written in these two ways: CH3COO- or CH3CO2 Since the acetate ion has a -1 charge, the manganese ion has a +4 charge state.
The phosphorus atom in PCl3 would be expected to have a partial positive (δ+) charge. partial negative (δ-) charge. 3+ charge. 3- charge.
partial positive (δ+) charge. Use the electronegativity trend and the periodic table as a visual tool: electronegativity increases up a group/family and across a period. Chlorine is more electronegative than phosphorus, so it will pull the electron density of the bond to itself, giving it the partial negative charge. Phosphorus yields to the greater pull (electronegativity) of chlorine, leaving it with a partial positive charge.
In a covalent bond, electrons are __________ between atoms. transferred shared pooled multiplied
shared
A triple bond between carbon atoms is _________ and _________ than a single bond between carbon atoms. longer, stronger longer, weaker shorter, stronger shorter, weaker Cannot be determined from this information
shorter, stronger Single bonds are longer than double bonds between atoms, and double bonds are longer than triple bonds. For Carbon bonding with another Carbon, this means that the order of bond length looks like this: C - C > C = C > C≡ C The more electrons pairs shared between atoms (double and triple bonds), the stronger the bond.
The more lone pairs on a central atom, such as the central atom of a molecule with a tetrahedral Electron Domain Geometry, the ____ the bond angle between the remaining peripheral atoms and the central atom.
smaller
What set of hybrid orbitals are used by the atom sulfur in the molecule SF4? sp sp2 sp3 sp3d sp3d2
sp3d 5 electron domains (s is implied as s1)
The set of hybrid orbitals used by bromine in BrF2- is: sp sp2 sp3 sp3d sp3d2
sp3d 5 electron domains (s is implied as s1)
The orbital hybridization on the iodine atom in ICl4— is A. sp B. sp2 C. sp3 D. sp3d E. sp3d2
sp3d2 6 electron domains= sp3d2 (s is implied as s1)
The set of hybrid orbitals used by bromine in BrF5 is: sp sp2 sp3 sp3d sp3d2
sp3d2 6 electron domains= sp3d2 (s is implied as s1)
According to the VSEPR theory, the electron domain geometry and the molecular geometry of the molecule BrF3 will be ________and ________, respectively.
trigonal bipyramidal, T-shaped
KCl in the solid state ___________ electricity, because ______________. will conduct, it is an ionic compound will not conduct, it is a covalent compound will not conduct, it is not dissolved in water will conduct, it is in the solid form.
will not conduct, it is not dissolved in water Ionic compounds have high melting and boiling pts, and will NOT conduct in the solid state. Conduction requires mobility of ions. Molten and aqueous ionic species will conduct, but in the solid state, the ions cannot move.
Predict the bond angles in the hydronium ion, H3O+, based on the VSEPR theory. ~90° ~104.5° ~107° ~109.5° ~120°
~107° Tetrahedral= ~109.5 w/ one lone pair= ~107
