CHEM UNIT 2 (Lecture)
How many electrons can the d orbital subshell hold?
10
How many electrons are in the 3rd shell in V+2?
11 V: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
How many orbitals does the P block have?
3
Which is bigger, 2s or 4s?
4s
What are the major species present in an aqueous solution of ethanol, CH3CH2OH(aq)?
CH3CH2OH and H2O
Which atom's valence electrons experience the greatest effective nuclear charge? a) Mg b) Ba c) Cl
Cl
How do you calculate pressure?
Force/Area
Write the molecular equation for the reaction between Ba(NO3)2and K2CO3.
K2CO3(aq) + Ba(NO3)2(aq) -> 2KNO3(aq) + BaCO3(s)
What would precipitate if you mixed potassium sulfate and lead (II) nitrate?
K2SO4(aq) + Pb(NO3)2(aq) -> 2KNO3(aq) + PbSO4(s)
Which is easier to ionize? (a) Li or (b) F
Li
What would precipitate if you mixed ammonium hydroxide and iron (III) chloride?
NH4OH(aq) + FeCl3(aq) -> NH4Cl(aq) + Fe(OH)3(s)
Do gases, liquids, solids, solids, and weak acids/bases break up in ionic equations?
NO
Would a solution of ethanol conduct electricity?
No, there are no ions.
Are there IMFs in ideal gasses?
No. Gas particles act independently of one another; no attractive or repulsive forces between particles.
Which of the following is correct? 1. All covalent substances dissolve in water. 2. All ionic substances are insoluble in water. 3. The table of solubility guidelines applies to both covalent and ionic compounds. 4. The term soluble implies that a substance dissolves in water and should be labeled (s)in a chemical formula or chemical reaction.
None of these.
The reduced species is the...
Oxidizing agent
Write net ionic equation for: Ammonium bromide and lead (II) nitrate react to form lead (II) bromide and ammonium nitrate
Pb+2(aq) + 2Br-1(aq) -> PbBr2(s)
Complete the reaction: Pb(NO3)2(aq) + 2KI ->
PbI2(s) + 2KNO3(aq)
What is a precipitation reaction?
Processes in which soluble ionic reactants yield an insoluble solid product that precipitates out of solution.
What is the order of the orbitals (letter ID)?
S, P, d, f
Do bases accept or donate H+?
accept
Which statement is correct? a) s orbitals are spherical in shape. b) p subshells hold a max of 6 electrons. c) All orbitals hold a max of 2 electrons.
all of the above
Which of the following does not have a noble gas electron configuration? a) Sc3+ b) As3- c) V3+ d) F-1
c) V = [Ar]4s^2 3p^3 so if loses 3 electrons, still has 2 before has noble gas configuration.
Do acids accept or donate H+?
donate
What is a net ionic equation
only reactants and products undergoing change are present
Do weak acids result in complete or partial dissociation?
partial
Do weak bases result in complete or partial reaction?
partial
Dissociation is a physical or chemical change?
physical
What is the Octet Rule?
tendency for bonded atoms to possess a complete outer shell to obtain stable electron configuration and lower their potential energy.
What is Daltons law of partial pressure?
the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Do weak acids have strong or weak electrolyte properties?
weak
Do weak bases have strong or weak electrolyte properties?
weak
How many moles of ions are produced when 1.0 mole of ammonium phosphate dissociates water?
(NH4)3PO4 = 3 NH4+1 + 1 PO4-3 = 4 mol ions
What is the oxidation number of sulfur in: SCl2
+2
What is the oxidation number of sulfur in: Na2SO3
+4
What is the oxidation number of Cr in K2Cr2O7?
+6
What is the oxidation number of sulfur in: SO4-2
+6
What is the oxidation number of sulfur in: H2S
-2
What is the oxidation number of sulfur in: Na2S
-2
What is the oxidation number of sulfur in: S-2
-2
Complete the reaction: HF(aq) + K2O(aq) -> Write the net ionic eq.
-> KF (aq) + H2O(l) Net Ionic: 2HF(aq) + O-2(aq) → 2F-1(aq) + H2O(l)
What is the oxidation number of sulfur in: S8
0
List the amount of aq ions produced when 0.1 moles AlCl3(aq) dissociate in pure water
0.1 mol Al+3 + 0.3 mol Cl-1
List the amount of aq ions produced when 0.1 moles MgCl2(aq) dissociate in pure water
0.1 mol Mg+2 + 0.2 mol Cl-1
How many orbitals does the S block have?
1
How many unpaired electrons are in an atom of bromine?
1
List the amount of aq ions produced when 1 mole Cu(CH3CO2)2 dissociate in pure water
1 mol Cu+2 + 2 mol acetate ions
How many electrons can the f orbital subshell hold?
14
How many electrons can each orbital hold?
2
How many electrons can the S orbital subshell hold?
2
How many valence electrons are in V? V: [Ar]4s23d3
2
List the amount of aq ions produced when 2 moles NaCl(aq) dissociate in pure water
2 mol Na+1(aq) + 2 mol Cl-1(aq)
Rank these solutions from LOWEST to HIGHEST electrical conductivity: 0.1 M NaCl 0.1 M AlCl3 0.1 M sucrose (C12H22O11) 0.1 M MgCl2
2, 4, 1, 3 more ions = more conductivity
How many ions are in 2.35 moles of sodium sulfide?
2.35 mol Na2S x 3 mol ion/1 mol Na2S = 7.05 mol ions
Write net ionic equation for: (NH4)2SO4 + AgNO3
2Ag+1(aq) + SO4-2(aq) -> Ag2SO4(s)
Write the complete ionic equation for the reaction between Ba(NO3)2and K2CO3. What are the spectator ions?
2K+1(aq) + CO3-2(aq) + Ba+2(aq) + 2NO3-1(aq) -> 2K+1(aq) + 2NO3-1(aq) + BaCO3(s) Spectator Ions: 2K+1(aq), 2NO3-1(aq)
How many particles result when Mg(ClO3)2 dissolves?
3 Mg+2 2ClO3-1
Predict the products of the acid-based reaction: Ba(OH)2(aq) + H3PO4 Balance the equation. Identify strong/weak acid and strong/weak base. Write net ionic equation.
3Ba(OH)2(aq) + 2H3PO4(aq) -> 3H2O(l) + Ba3(PO4)2(s) Strong base: Ba(OH)2(aq) Weak acid: H3PO4(aq) Net ionic: 3Ba+2(aq) + 2OH-1(aq) + 2H3PO4(aq) -> 3H2O(l) + Ba3(PO4)2(s)
What is the total concentration of ions in a 1.0 molar solution of ammonium phosphate?
4 mol ions / 1.0 L = 4.0 M
Rank these four solutions by increasing conductivity from LOWEST (1) to HIGHEST (4): 1.0 M Na2S(aq) 1.0 M HNO3(aq) 1.0 M HF(aq) 1.0 M CH3OH(aq)
4, 3, 2, 1
How many orbitals does the d block have?
5
What is the concentration (in M)of a solution made by dissolving 5.0 mole of sodium chloride in 1.5 L of water?
5.0 mol NaCl / 1.5 L = 3.3 M NaCl (aq)
How many electrons can the P orbital subshell hold?
6
What is the total concentration of ions in a 2.35 molar solution of sodium sulfide?
7.05 mol ions / 1L = 7.05 M
How many valence electrons are in an ion of Ca?
8 Ca atom: [Ar]4s2 Ca ion (Ca+2): [Ar] Ca ion (Ca+2): [Ne]3s^2 3p^6
What is an amphiprotic molecule?
A molecule that can either accept or donate a proton, depending on what it meets. Ex: H2O
What is Electron Affinity?
Adding e- to neutral (g) atom often RELEASES E (-) (releases energy)
Which is the correct order for highest to lowest conductivity for equal concentrations of aqueous solutions of the following: AlBr3, BaS, CH3CH2OH, K2S
AlBr3 > K2S > BaS > CH3CH2OH 4, 3, 2, 0 ion/unit
Molarity is a conversion factor between volume and moles for...
Aqueous solutions
Which has the larger radius? (a) Mg (b) Ba (c) Cl
Ba
Which is easier to ionize? (a) Mg or (b) Ba
Ba
Predict the products of the acid-based reaction: Ba(OH)2(aq) + CH3CO2H Balance the equation. Identify strong/weak acid and strong/weak base. Write net ionic equation.
Ba(OH)2(aq) + 2CH3CO2H(aq) -> 2H2O(l) + Ba(CH3CO2)2(aq) Strong base: Ba(OH)2(aq) Weak acid: CH3CO2H(aq) Net ionic: OH-1(aq) +CH3CO2H(aq) -> H2O(l) + CH3CO2-1(aq)
Write the net ionic equation for the reaction between Ba(NO3)2and K2CO3. What are the spectator ions?
Ba+2(aq) + CO3-2(aq) -> BaCO3(s)
Write net ionic equation for: Nickel (II) sulfate and barium chloride are mixed to produce nickel (II) chloride and barium sulfate.
Ba+2(aq) + SO4-2(aq) -> BaSO4(s)
What is/are the spectator ions? Mg(s) + 2HBr(aq) -> MgBr2(aq) + H2(g)
Br-1
What are the two primary chemical species present in a 1.0 M aqueous solution of ethanol? Are there any ions?
CH3CH2OH(aq) and H2O(l) No ions
Write net ionic equation for: Ca(NO3)2 + Na2CO3
Ca+2(aq) + CO3-2(aq) -> CaCO3(s)
Write net ionic equation for: Li2S + Co(NO3)2
Co+2(aq) + S-2(aq) -> CoS(s)
Write net ionic equation for: Cu(OH)2 + HNO3
Cu(OH)2(aq) +2H+1(aq) -> Cu+2(aq) + 2H2O(l)
What is the trend in first ionization energy down the periodic table (vertical)? Why?
E decreases (easier to ionize) mostly due to shell #
What are trends in effective nuclear charge down the periodic table (vertical)?
Effective nuclear charge (Zeff) decreases Nuclear charge increases Distance from nucleus (shell #) increases
What are trends in effective nuclear charge across the periodic table (horizontal)?
Effective nuclear charge (Zeff) increases Nuclear charge increases Shielding by inner e-mostly constant.
True or False: Acetic acid (CH3CO2H) is a strong electrolyte.
False
True or False: All acids are strong electrolytes.
False
True or False: CH3OH (methanol, at right) is a weak acid.
False
True or False: Nitric acid is a weak electrolyte.
False
Write net ionic equation for: HNO3 + CsOH
H+1(aq) + OH-1(aq) -> H2O(l)
A balloon is filled with hydrogen and oxygen. Which leaks out faster?
H2 because it has less mass
What is produced by acids in an acid-based reaction?
H3O+
What is the trend in first ionization energy across the periodic table (horizontal)? Why?
IE increases (harder to ionize) Mostly due to Zeff
What happens to ionization energy as remove more e-?
Increase
What is being broken apart when ethanol, CH3CH2OH, dissolves in water to make liquor?
Intermolecular Forces (IMFs)
What unit must temperature be in for gas laws?
Kelvin
If an element is easier to ionize, does it require more or less energy?
Less
Are the metals at the top or bottom of the Activity Series least reactive?
Metals at the bottom
Do the metals at the top or bottom of the Activity Series most want to give up e- ?
Metals at the top
What is the reducing agent? Mg(s) + 2HBr(aq) -> MgBr2(aq) + H2(g)
Mg
What undergoes oxidation? Mg(s) + 2HBr(aq) -> MgBr2(aq) + H2(g)
Mg
Determine the molecular, total ionic, and net ionic reactions if the weak base, NH3and strong acid, HClO4, react.
Molecular: NH3(aq) + HClO4(aq) -> HN4+1(aq) + ClO4-1(aq) Total Ionic: NH3(aq) + H+1(aq) + ClO4-1 -> NH4+1(aq) + ClO4-1(aq) Spectator Ions: ClO4-1 Net Ionic: NH3(aq) + H+1(aq) -> NH4+1(aq)
What is the octet rule?
Most stable form of atom or ion is with complete outer shell/valence shell
Which of the following is correct? 1. The substance in the smaller amount in a solution is called the solvent. 2. Calcium phosphate, Ca3(PO4)2, is soluble in water. 3. All covalent compounds are soluble in water. 4. NaCl(aq) is an electrolyte solution 5. CaCl2(aq) produces two ions/formula unit.
NaCl(aq) is an electrolyte solution
According to the Activity Series, will the reaction go? CO(s) + ZnNO3 -> ??
No
Do covalent compounds dissociate in water?
No
Solid lead is placed in a solution of nickel (II) chloride. Will a reaction occur? If so, write a balanced chem. eq.
No Pb(s) + NiCl2(aq) -> NR Pb is less active than Ni (Ni wants to give up e-, Pb wants to keep it's e-)
Write net ionic equation for: Sr(C2H3O2)2 + KBr
No Reaction
Complete the reaction: KI(aq) + NaCl(aq) ->
No reaction
Do covalent compounds have strong or weak electrolytes?
None- Non Electrolyte (excluding acids and bases)
Explain effective nuclear charge (Zeferino) vs nuclear charge
Nuclear charge is the total positive charge of all protons in the nucleus. Effective nuclear charge is the nuclear charge experienced by outer shells.
What is produced by bases in an acid-based reaction?
OH-
How many species in a reaction undergo redox?
Only 2 species
What is a molecular equation?
Overall reaction: all reactants and products in compound form
What is the trend in atomic radius across the periodic table (horizontal)? Why?
Radius decreases Mostly due to Zeff
What is the trend in atomic radius down the periodic table (vertical)? Why?
Radius increases Mostly doe to shell #
The oxidized species is the...
Reducing agent
What is Ionization Energy?
Removing e- from neutral (g) atom REQUIRES E (+) (requires energy)
Which trends are more pronounced, row or column?
Row trends
Once Na becomes Na+1, has same electron configuration as Ne (1s22s22p6) why doesn't Na+1 react same as Ne?
Same number of electrons but number of protons (and neutrons) are different and so is ratio of protons to electrons (charge).
What is similar and different about a row/period on the periodic table?
Similar: same number of inner shell electrons Different: different number valence electrons
What is similar and different about a column/group on the periodic table?
Similar: same number of valence electrons - similar reactivity! Different: different number inner shell electrons
Do ionic compounds have strong or weak electrolytes?
Strong- the more ions, the stronger
4s fills before 3d?
True
The p orbitals in the 3rd shell have the same energy?
True
True or False: All weak acids are weak electrolytes.
True
True or False: CH3OH(methanol) is a non-electrolyte.
True
True or False: Hydrofluoric acid is a weak electrolyte.
True
What are electrons in outer most energy level called?
Valence electrons
What are the only electrons that participate in chemical reactions
Valence electrons
According to the Activity Series, will the reaction go? CO3(s) + HNO3 -> ??
Yes
Solid nickel is placed in a solution of lead (II) acetate. Will a reaction occur? If so, write a balanced chem. eq.
Yes Ni(s) + Pb(CH3CO2)2 (aq) -> Ni(CH3CO2)2(aq) + Pb(s) Ni is more reactive than Pb (Pb wants to gain e- relative to Ni)
Can the same molecule act as an acid or a base, depending on what other substance it meets?
Yes- H2O can either accept or donate a proton, depending on the reaction.
What do "Z" and "S" represent in the effective nuclear charge equation?
Z = number of protons S = number of core electrons (shielding electrons)
What is the equation for effective nucelar charge?
Zeff= Z-S
Which of the following correctly illustrates the valence electron configuration of sulfur?
a
Anion - electron(s) _____________ __________ valence shell
added to
What is a complete ionic equation?
aq reactants/products in ion form solid, liquid, and gas in compound form spectator ions detected
What are degenerate orbitals?
atomic orbitals with the same name have the same energy
Which of the following is the correct electron configuration for bromine (Br)? a) 1s22s22p63s23p64s24d104p5 b) 1s22s22p63s23p64s23d104p5 c) 1s22s22p63s23p64s23d104p6 d) 1s22s22p63s23p64s24p6 e) 1s22s22p63s23p54s24p5
b) 1s22s22p63s23p64s23d104p5
What is the ground state electron configuration for V? a) V: [Kr]4s33d2 b) V: [Kr]4s24d3 c) V: [Ar]4s23d3 d) V: [Ar]3d3 e) V: [Kr]4s24d3
c) V: [Ar]4s23d3
Do strong acids result in complete or partial dissociation?
complete
Do strong bases result in complete or partial reaction?
complete
What is first ionization energy?
energy needed to remove ONE outermost e- from neutral atom in the gaseous state.
Is reducing losing or gaining an electron?
gaining an electron (becoming more negative)
Under what condition do atoms lose e-?
if they react with substance that wants e- more
Is oxidizing losing or gaining an electron?
losing an electron (becoming more positive)
What is effective nuclear charge?
nuclear charge actually felt by any electron.
s and p orbitals are ALWAYS...
outer shell/valence!
The species undergoing oxidation or reduction must be "higher" in the activity table in order for reaction "to go."
oxidation
Cation - electron(s) _____________ __________ valence shell
removed from
Molar mass is the conversion factor between mass and moles for...
solids
Do strong acids have strong or weak electrolyte properties?
strong
Do strong bases have strong or weak electrolyte properties?
strong
