Entrance Exam Semmelweis EXAM LATEST (2025) COMPLETE
Entrance Exam Semmelweis
QUESTIONS With 100% Verified Solutions,
Study online at https://quizlet.com/_bmpmf3
1. Electron configu- Subtract 1 from exponent of highest n-value orbital (ex. remove from 4s before
ration for cations 3d)
Ag+ = [Kr]5s^1 4d^9
2. Electron configu- Add 1 to closest orbital
ration for anions
Cl- = [Ne]3s^2 3p^6
3. Atomic orbitals s, p, d, f
4. Primary vs sec- Primary - AA chain (linked by peptide bonds)
ondary struc-
tures of proteins Secondary - stabilized by non-covalent bonds (alpha helices & beta sheets)
5. Most bonds in covalent
organic com-
pounds are
6. Properties of wa- 1. polar
ter 2. capable of adhesion and cohesion
3. high heat capacity (so it's hard to raise its temp)
4. great solvent
5. high heat of vaporization (allows humans to cool off via sweat)
6. water is less dense as a solid than a liquid
7. Intermolecular hydrogen bonding
forces of water
8. Solution compo- 1. solvent (product being dissolved)
nents 2. solute (medium for dissolving solvent)
9. Molarity the number of moles of solute per liter of solution
, Entrance Exam Semmelweis
Study online at https://quizlet.com/_bmpmf3
10. Solubility rules SOLUBLE
1. alkali metals (group 1) & NH4+ cations
2. NO3- or CH3COO- anions
3. Cl, Br, I (except when bonded to Ag+, Pb2+ or Hg2+)
4. sulfate ions (except when with Ca2+, Sr2+, Ba2+, Pb2+)
INSOLUBLE
1. Metal oxides (except CaO, SrO, BaO)
2. Hydroxides (except when with Ca2+, Sr2+, Ba2+)
3. Carbonates, phosphates, sulfides, and sulfites (unless bound to alkali metal or
NH4+)
11. Solubility prod- Ksp = [A]^a[B]^b
uct
**only products because we don't include solids in the equilibrium expression
for NaCl
- Ksp = x^2
for PbCl2
- Ksp = 4x^3
for Cr(OH)3
- Ksp = 27x^4
12. Large Ksp means strong electrolyte (more soluble)
13. Strong acids So I brought no clean clothes
1. H2SO4
2. HI
3. HBr
4. HNO3
5. HCl
, Entrance Exam Semmelweis
Study online at https://quizlet.com/_bmpmf3
6. HClO4
7. HClO3
14. Strong bases 1. NaOH
2. LiOH
3. KOH
4. CsOH
5. RbOH
6. Ba(OH)2
7. Ca(OH)2
8. Sr(OH)2
Bases can certainly look pleasing (K), really something strong (Na)
15. Le Chatlier's prin- pressure applied (or volume reduced) --> equilibrium proceeds in direction with
ciple: pressure fewer moles
pressure removed (or volume increased) --> equilibrium proceeds in direction
with more moles
16. Le Chatlier's prin- increasing temperature
ciple: tempera- - toward products (if endothermic)
ture - toward reactants (if exothermic)
decreasing temperature
- toward products (if exothermic)
- toward reactants (if endothermic)
17. Le Chatlier's prin- increase concentration of reactants
ciple: concentra- - reaction shifts toward products
tion
decrease concentration of reactants
- reaction shifts toward reactants
Entrance Exam Semmelweis
QUESTIONS With 100% Verified Solutions,
Study online at https://quizlet.com/_bmpmf3
1. Electron configu- Subtract 1 from exponent of highest n-value orbital (ex. remove from 4s before
ration for cations 3d)
Ag+ = [Kr]5s^1 4d^9
2. Electron configu- Add 1 to closest orbital
ration for anions
Cl- = [Ne]3s^2 3p^6
3. Atomic orbitals s, p, d, f
4. Primary vs sec- Primary - AA chain (linked by peptide bonds)
ondary struc-
tures of proteins Secondary - stabilized by non-covalent bonds (alpha helices & beta sheets)
5. Most bonds in covalent
organic com-
pounds are
6. Properties of wa- 1. polar
ter 2. capable of adhesion and cohesion
3. high heat capacity (so it's hard to raise its temp)
4. great solvent
5. high heat of vaporization (allows humans to cool off via sweat)
6. water is less dense as a solid than a liquid
7. Intermolecular hydrogen bonding
forces of water
8. Solution compo- 1. solvent (product being dissolved)
nents 2. solute (medium for dissolving solvent)
9. Molarity the number of moles of solute per liter of solution
, Entrance Exam Semmelweis
Study online at https://quizlet.com/_bmpmf3
10. Solubility rules SOLUBLE
1. alkali metals (group 1) & NH4+ cations
2. NO3- or CH3COO- anions
3. Cl, Br, I (except when bonded to Ag+, Pb2+ or Hg2+)
4. sulfate ions (except when with Ca2+, Sr2+, Ba2+, Pb2+)
INSOLUBLE
1. Metal oxides (except CaO, SrO, BaO)
2. Hydroxides (except when with Ca2+, Sr2+, Ba2+)
3. Carbonates, phosphates, sulfides, and sulfites (unless bound to alkali metal or
NH4+)
11. Solubility prod- Ksp = [A]^a[B]^b
uct
**only products because we don't include solids in the equilibrium expression
for NaCl
- Ksp = x^2
for PbCl2
- Ksp = 4x^3
for Cr(OH)3
- Ksp = 27x^4
12. Large Ksp means strong electrolyte (more soluble)
13. Strong acids So I brought no clean clothes
1. H2SO4
2. HI
3. HBr
4. HNO3
5. HCl
, Entrance Exam Semmelweis
Study online at https://quizlet.com/_bmpmf3
6. HClO4
7. HClO3
14. Strong bases 1. NaOH
2. LiOH
3. KOH
4. CsOH
5. RbOH
6. Ba(OH)2
7. Ca(OH)2
8. Sr(OH)2
Bases can certainly look pleasing (K), really something strong (Na)
15. Le Chatlier's prin- pressure applied (or volume reduced) --> equilibrium proceeds in direction with
ciple: pressure fewer moles
pressure removed (or volume increased) --> equilibrium proceeds in direction
with more moles
16. Le Chatlier's prin- increasing temperature
ciple: tempera- - toward products (if endothermic)
ture - toward reactants (if exothermic)
decreasing temperature
- toward products (if exothermic)
- toward reactants (if endothermic)
17. Le Chatlier's prin- increase concentration of reactants
ciple: concentra- - reaction shifts toward products
tion
decrease concentration of reactants
- reaction shifts toward reactants
