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Chemistry
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Questions in this quiz (100)
1On the matter we can say:
- Aevery form of its existence is expressed by the movement in the space and time
- Bit exists in the form of fields
- Cit can be changed from the substance to the field
- Dit exists in infinite numbers of different forms
2If NaCl is dissolved is destilled water, following item arises:
- Acolourless solution
- Bclosed system
- Ctrue solution
- Dsolution of electrolyte
3Drinking water is:
- Atrue solution
- Bconsists only of molecules oh h2o
- Chomogenous substance
- Dgood solvent of ionic compounds
4Solution of protein in water:
- Ais not true solution
- Bis colloidal solution
- Cis chemically pure substance
- Dis true solution
5Elementary structural unit of the substance is:
- Aproton
- Belectron
- Catom
- Dnucleon
6Pure substance can be:
- Asolution of NaCl is destilled water
- Bonly a compound
- CAl2o3
- Delectron
7Proton is particle which:
- Ahas one elementary positive charge
- Bhas one elementary negative charge
- Cdoes not belong among nucleous
- Dbelongs among nucleous
8Nuclides 1H1, 2H1 and 3H1:
- Aare isotopes
- Bhave the same number of protons
- Chave the same amount of neutrons
- Dhave different amount of nucleons
9Nuclides 16 O 8, 17 O 8 and 18 O 8:
- Acan be found in the nature in the same amount
- Bhave the same number of neutrons
- Chave the same number of nucleons
- Dare isotopes
10Maximum number of electrons in subshell with principal quantum number (shell) n=2 is:
- A2
- B8
- C18
- D32
11Subshell M can posses:
- Amaximum 16 electrons
- Bonly p orbital types
- Conly s and p orbitals
- Ds, p, d oribitals
12Neutron:
- Ais a particle the mass of which is approximately equal to the mass of hydrogen molecule
- Bis a particle which has only one elementary positive charge
- Cis electrically uncharged (neutral) particle
- Dhas the mass approximately equal to the proton
13According to the Pauli's principal:
- Ain the orbital Px can be maximum 1 electron
- Bin the orbital Py can be maximum 2 electrons
- Cin the orbital Py can be maximum 6 electrons
- Din the orbital Pz can be maximum 10 electrons
14Energy needed for the cleavage of a certain chemical bond:
- Ais the same as the activation energy
- Bis the same as energy which is released during its formation
- Cis bigger than energy which is released during its formation
- Dis the same as ionization energy
15In molecule of acetylene between carbon atoms:
- Athere are 3 sigma bonds
- Bthere is 1 sigma and 2 pi bonds
- Cthere are 2 sigma and 1 pi bonds
- Dthere are covalent bonds
16Triple bond:
- Ain a molecule of hydrocarbon is more reactive than simple
- Bamong the equal atoms is the strongest
- Cis typical for alkadienes
- Darises by covering of s orbitals
17ionic compounds:
- Amajority of them are not soluble in water
- Bmajority of them are soluble in water
- Chave the structure where cations and anions are attracted by eletrostatic forces
- Das meltings or in solutions are conducting eletric current
18Electronegativity of potassium atom is 0.9 and bromine atom is 2.7. What type of bond is between atoms of Br and K in KBr:
- Api bond
- Bdouble bond
- Csigma bond
- Dionic bond
19Cations are ions which:
- Aare moving in electric field to he cathode
- Bhave positive charge
- Care moving in electric field to anode
- Dcannot be formed from atoms of alkali metals
20If both electrons of the covalent bond are contributed only by one atom we can call this bond:
- Acoordinate covalent
- Bdonor-acceptor
- Cmetal
- Dcovalent nonpolar
21In molecule of NH4Cl among individual atoms there can be following bonds:
- Aionic
- Bcoordinate-covalent
- Ccovalent
- Dhydrogen bond (H bond)
22Nonpolar molecule is:
- ACO
- BCO2
- CN2
- DCH3CH2OH
23Single covalent bond:
- Ais between aloms C-C and C-H of alkanes
- Bis in molecule H2
- Cis created if difference of eletronegativity between atoms is bigger than 1.7
- Dis e.g in molecule of NaCl
24Hydrogen bond:
- Ais named hydrogen bridge
- Bis stronger than covalent bond
- Cis created between molecules (groups) which have atoms of hydrogen bound with strong electronegative elements (mainly F, O, N)
- Dis created in molecules of proteins
25In simple proteins are present bonds:
- Acovalent
- Bhemiacetal
- Cester
- Dhydrogen bonding
26Hydrogen bonds are formed:
- Ain molecules of DNA
- Bamong molecules of H2O
- Camong molecules of NH3
- Damong molecules of CH4
27Van der Waals forces:
- Aare created among anions and cations
- Bare based on mutual effects of molecular dipoles
- Care 100 times weaker than covalent bonds
- Dare in complex compounds
28What are the oxidation numbers of elements in listed oxides if oxidation number of oxygen atom is -II: Mn2O7, HgO, Ag2O, P4O6, N2O5, SO3, SiO2:
- AV, I, II, III, V, IV, VI
- BVII, II, II, III, V, VI, IV
- CVII, II, I, III, V, IV, VI
- DVII, I, II, II, V, IV, VI
- ENENHUMA
29Eletronegativity:
- Aof alkali metals is low
- Bis high in elements which create cations very easily
- Cof elements F, Cl, Br, I is high
- Dis proportional to the energy released during creation of anion from an atom in gaseous state
30In molecules of starch are bonds:
- Aalpha (1-4) glycosidic
- Balpha (1-6) glycosidic
- Cbeta (1-4) glycosidic
- DN-glycosidic
31In molecule of CH2=CH2 are bonds:
- A2 sigma bonds and 2 pi bonds
- B1 sigma bond and 1 pi bond
- C5 sigma bonds and 1 pi bond
- D1 sigma bond and 3 pi bonds
32Double bond:
- Ais created by sigma and pi bond
- Bis created by one pair of electrons
- Ccan be found in molecules of long-chain fatty acids
- Dcan be conjugated
33Peptide bond:
- Ais amide bond in peptides
- Bcan be cleaved by hydrolases
- Cis formed in a process of proteosynthesis
- Dbelongs to weak bonds
34Glycosidic bonds:
- Aalpha (1-4) are also in molecule of starch
- Bare formed during oxidation of saccharides
- Calpha (1-6) are in molecule of glycogen
- Dcan be O-glycosidie
35According to the Brönsted theory acids are:
- Asubstances which are able to release proton
- Bsubstances which are acceptors of proton
- Csubstances which are able to release atom of hydrogen
- Dsubstances which can release H2
36According to the Brönsted theory bases are:
- Acompounds which are able to release proton
- Bacceptors of proton
- Ccompounds which are able to accept H+
- Dall compounds which have -OH group in molecule
37What are conjugated pairs of protolytic reaction HNO3 + H2O <-> H3O+ + NO3- :
- AHNO3 and NO3-
- BH2O and NO3-
- CH3O+ and NO3-
- DH2O and H3O-
38Determine conjugated bases of protolytic reaction CH3COOH + C6H5NH2 <-> C6H5NH3+ + CH3COO- :
- Aaminobenzene and C6H5NH3+
- BCH3COOH and CH3COO-
- CC6H5NH3+ and CH3COO-
- Dethanoic acid and CH3COO-
39Strength of acids decreases in order: HClO4 > HClO3 > HClO2 > HClO. Then following statement is valid:
- Apolarity of bonds O-H increases
- Bvalue of pK of acids increases
- Cvalue of ionization (dissociation) constant decreases
- Dall values of ionization constants (K) are the same
40For solutions of eletrolytes following statement is true:
- Aat the same concentration (mol.l -1) they have lower osmotic pressure than solutions of noneltrolytics
- Btheir concentration can be expressed only in mol.l -1
- Cthey have freely movable ions
- Dthey do not undergo electrolysis
41Strength of acids and bases:
- Aare judged according to the solvent in which they are prepared
- Bare determined according to the value of osmotic pressure pi of acid or base solution
- Care determined according to the value of their ionization constant
- Dare determined according to the value of their isoelectric point
42Acidic reaction has solution if:
- ApH= 4.8
- BpOH= 11.9
- CpOH > 7
- DpH < 6
43Alkaline reaction has solution if:
- ApOH < 7
- BpH > 6
- CpOH = 4.5
- DpOH > 7
44Alkaline reaction has solution if:
- Ac(H3O+) = 2 x 10-8 mol.l -1
- Bc(OH-) = 7 x 10-10 mol.l -1
- Cc(H3O+) = 1 x 10-7 mol.l -1
- Dc(H3O+) = 7 x 10-1 mol.l -1
45Acidic reaction has solution if:
- Ac(OH-) = 4 x 10-12 mol.dm -3
- Bc(H3O+) = 7 x 10-5 mol.dm -3
- Cc(OH-) = 3 x 10-5 mol.dm -3
- Dc(H3O+) = 7 x 10-10 mol.dm -3
46If ionization constant of nitrous acid is 4.5 x 10-4, (log 4.5= 0.65) then following statement is true:
- Anitrous acid is weak acid
- Bnitrous acid is strong acid
- Cnitrous acid is weak electrolyte
- Dsolution of HNO2 reacts only with weak bases
47Ionization constant of a base:
- Ahas always the same value as ionization constant of conjugated acid
- Bhas always the same value as autoprotolytic constant of water
- Ccharacterizes the ability to attract proton
- Ddetermines the strenght of a base
48Acidity of the solution, characterized by pH or pOH increases in order:
- Aph 7 < ph 5 < ph 2 < ph 1
- Bph 14 < ph 7 < ph 6 < ph 5
- Cpoh 13 < poh 12 < poh 11 < poh 10
- Dph 12 < ph 11 < ph 10 < ph 9
49Alkaline solutions are characterized by pH or pOH, basicity increases in order:
- Aph 7 < ph 8 < ph 9 < ph 10
- Bph 3 < ph 4 < ph 5 < ph 6
- Cph 14 < ph 12 < ph 11 < ph 10
- Dpoh 8 < poh 6 < poh 3 < poh 1
50Alkaline reaction give following pairs of aqueous solutions of salts:
- ACH3COONa, KCN
- BNH4Cl, CH3COONH4
- CFe2(SO4)3, Na2SO4
- DCH3COOK, Na2S
51Acidic reaction give following pair of aqueous solutions:
- AK2S, Ca(HCO3)2
- BCH3COONa, Na3PO4
- C(NH4)2SO4, Fe(NO3)3
- DKCN, KNO3
52Which of salt pairs solutions are almost not hydrolyzed:
- AK2SO3, BiCl3
- BRbCl, Na2SO4
- CNaCN, (NH4)2S
- DLi2SO4, NaClO4
53According to the Bronsted theory acids can be:
- Ae.g. ions HCO3-, HSO4-, OH-, PO4 3-
- Bonly electroneutral molecules
- Conly cations, e.g. NH4 +
- Delectroneutral molecules, cations and anions, which can split off H+
54Strong and weak bases differ each other by:
- Athe amount of -OH groups which can accept from other molecules
- Bthe solubility in water
- Cthe concentration in non-aqueous solvents
- Dthe amount of - OH groups in a molecule
- ENENHUMA
55Choose groups of compounds which in aqueous solution are electrolytes:
- ACoCl2, Na2CO3, CHCl3, HCl, C2H6
- BCH4, benzene, KmnO4, CH3COOH, K2SO4
- CFeCl3, H2SO4, NaBr, CH3COOK, NH4Br
- DCuSO4, H2O, HI, NaNO3, K3[Fe(CN)6]
56Mark compounds which cause decrease of pH after dissolution in water (pH water= 7):
- ACaO, BaCl2
- BSO2, NH4Cl
- Cethanol, MgO
- D(NH4)2SO4, CH3COOH
57True solutions are:
- Aonly solutions of strong electrolytes
- Bthose, in which size of dissolved particles is bigger than 1 x 10 *9- m
- Ccrude dispersion systems of liquid and solid substance
- Dhomogenous mixtures of gas and solid substance
- ENenhuma
58In true solutions size of dissolved particle is:
- A1 - 10² mm
- B1 - 10 micro m
- Cless than 1 nm
- D10 - 100 nm
59Choose pairs of aqueous solutions of strong electrolytes:
- AMgCl2, KOH
- BCsOH, NH4OH
- CNaOH, SnSO4
- DHCl, K2CrO4
60Choose pairs of aqueous solutions of weak electrolytes:
- ACoCl2, Na2SO3
- BNiCl2, NH4OH
- CNa2CO3, H2CO3
- DHCOOH, HNO3
61Weak electrolytes:
- Ahave value of ionization constant a =1
- Bthey differ from strong electrolytes by dissociation constants
- Cthey are present in solutions only in the form of ions
- Dthey have the same value of pK as strong electrolytes
62There are given 3 water solutions, mark, which of statements is correct:
A (NiCl2), e=0.1 mol.l¹-;
B (KCl), e=0.15 mol.l¹-;
C (sucrose), e=0.3 mol.l¹-;- Athe greatest osmotic pressure is in solution C
- Bin solution A is the lowest osmotic pressure
- Cin all solutions is equal osmotic pressure
- Dsolution B has greater osmotic pressure than solution A
63There is solution of NaCl (e=0.1 mol.l¹-). Mark which of solutions are isotonic to the solution of NaCl:
- ACuSO4, e=0,1 mol.l¹-
- Bfructose, e=0.3 mol.l¹-
- CNiCl2, e=0.15 mol.l¹-
- DCdSO4, e=0.15 mol.l¹-
64There is solution of Ba(NO3)2 with concentration 0.2 mol.l¹-. Mark which of solutions are hypertonic to the solution of Ba(NO3)2:
- AAgNO3, e= 0.5 mol.l¹-
- BFeSO4, e= 300 mmol.l¹-
- CFe2(SO4)3, e=0.15 mol.l¹-
- DNiCl2, e= 300 mmol.l¹-
65Saline is an aqueous solution of NaCl (Mr=58) with concentration 0.15 mol.l¹-. This solution contains:
- A30 mmol of NaCl in 200 ml of solutions
- B0.15 mol of NaCl in one litre of H2O
- C17.4g of NaCl in 2L of solution
- D4.35g of NaCl in 500 ml of H2O
66Osmosis:
- Ais the process which cannot proceed in human organism
- Bis characteristic for the system formed by solvent, solution and semi permeable membrane between them
- Chappens when two solutions of NaCl with different concentrations are separated by semi permeable membrane
- Dis free movement of particles of dissolved compound from the place of higher concentration to the place of lower concentration
67Oxidation:
- Ais every chemical reaction during which either atoms or ions of elements accept electrons
- Bis every chemical reaction during which either atoms or ions of elements lose electrons
- Cis the process during which positive oxidation number of atoms decreases
- Dis the process during which positive oxidation number of atoms increases
68Reduction:
- Ais every chemical reaction during which either atoms or ions of elements accept electrons
- Bis every chemical reaction during which either atoms or ions of elements lose electrons
- Cis the process during which positive oxidation number of atoms decreases
- Dis the process during which negative oxidation number of atoms increases
69Reducing agents are compounds which:
- Aare donors of electrons in chemical reaction
- Bare acceptors of electrons in chemical reaction
- Care donors of protons in chemical reaction
- Dare donors of hydrogen atoms during hydrogenation of the other compounds
70Oxidizing agents are compounds which:
- Aare acceptors of protons in chemical reaction
- Bare acceptors of hydrogen atoms in dehydrogenation of compounds
- Cduring oxidation-reduction reaction accept electrons
- Dare donors of electrons in chemical reaction
71Mark which of following compounds can act as oxidizing agents in chemical reactions:
- AHNO3
- BKClO3
- CK2Cr2O2
- DKMnO4
72Dismutation is reaction:
- Aoxidation-reduction
- Bduring which one substance (molecules of the same compound, the same ions or atoms of the same element) gain and lose electrons
- Cduring which the same ions or atoms of the same element undergo both oxidation and reduction
- DCl2 + H2O -> HClO + HCl
73Iodine atom has oxidation number VII in compounds:
- ANaIO
- BI2O2
- CPbI2
- DNH4I
74Chromium atom has oxidation number VI in compounds:
- ACr2O3
- BKCr(SO4)2 . 12 H2O
- CCr(OH)3
- DK2CrO4
75Iron atom has oxidation number III in compounds:
- AFe(SCN)3
- B(NH4)Fe(SO4)2 . 6 H2O
- CFe(CH3COO)3
- DNH4Fe(SO4)2 . 12 H2O
76Oxygen atom has oxidation number -1 in compounds:
- ANa2O2
- BBaO
- CK2O2
- DBaO2
77Manganese atom has oxidation number VII in compounds:
- AMnSO4
- BCa(MnO4)2
- CMn2O7
- DKMnO4
78Atom of sulphur has oxidarion number -II in compounds:
- AH2S
- BCO2(SO4)3
- CSb2S5
- DMg(HS)2
79About chemical reaction Mg + NiCl2 <--> MgCl2 + Ni can be stated:
- Amagnesium is reduced
- Bchlorine is reduced
- Caction Ni2+ is reduced
- Dcation Ni2+ is oxidized
80About reaction Fe + CuSO4 <--> FeSO4 + Cu we may say:
- Airon is oxidized
- Bcooper is oxidized
- Cit is oxidation-reduction reaction
- Doxidation number of cooper is not changed
81About reaction Zn + CuSO4 <--> ZnSO4 + Cu we can say:
- Acupric cation is oxidized
- Bcation Cu2+ is oxidizing agent
- Cit is oxidation-reduction reaction
- Doxidation numbers of atoms are not changed
82About reaction Fe + 2 HCl (diluted) --> FeCl2 + H2 we can say:
- AFe is oxidized
- BFe is reduced
- Cit is oxidation-reduction reaction
- Dchloride anion is oxidized
83About reaction Zn + H2SO4 (diluted) --> ZnSO4 + H2 we can say:
- Acations of hydrogen are reduced
- Bzinc is reduced
- Creaction is oxidation-reduction reaction
- Dsulphur is reduced
84About reaction Cu + H2SO4 (conc.) --> CuO + SO2 + H2O we can say:
- Asulphur is oxidized
- Bcations H+ are reduced
- Ccations H+ are oxidized
- Danions SO4²- acts as oxidizing agent
85Potassium atom in reaction 2K + 2 H2O --> 2 KOH + H2:
- Ais reducing agent
- Bis reduced
- Cis oxidized
- Dis oxidizing agent
86Iodine is oxidized in reactions:
- ACl2 + 2 KI --> I2+ 2KOH + O2
- B2 KI + O3 + H2O --> I2 + 2 KOH + O2
- C3 I2 + 10 HNO3 --> 6 HIO3 + 10 NO + 2 H2O
- DNaIO3 + NaClO --> NaIO4 + NaCl
87Sulphur is oxidized in reaction:
- AFe2S3 + 4 HCl --> 2 FeCl2 + 2 H2 + 3 S
- B2 Cr + 6 H2SO4 --> Cr2(SO4)3 + 3 SO2 + 6 H2O
- CI2 + H2S --> 2 HI + S
- DNaOH + SO2 --> NaHSO3
88Mark reactions in which H2O2 is oxidizing agent:
- AH2O2 + 2 FeSO4 + H2SO4 --> Fe2(SO)4 + 2H2O
- B5 H2O2 + 2 KMnO4 + 3 H2SO4 --> 5 O2 + 2 MnSO4 + K2SO4 + 8 H2O
- CH2O2 + PbO2 + 2HNO3 --> Pb(NO3)2 + O2 + 2 H2O
- DH2O2 + 2 Kl + H2SO4 --> l2 + K2SO4 + 2 H2O
89Rate of chemical reaction:
- Ain gases depends on their pressure
- Bdepends on the concentration of reacting components
- Cis influenced by catalysts
- Dis directly proportional to the concentration of reacting substances
90Equilibrium state of the reaction:
- Ais the state when reaction proceeds at the same rate in both directions
- Bis the state when reactants are completely changed to products
- Cis expressed by equilibrium constant
- Dis the state when concentrations of reactants in reaction mixture are the same as concentrations of products.
91Chemical equilibrium of reaction 2HBr <--> H2 + Br2 with value of reaction heat Qm= + 70 kJ.mol¹- changes to the side of reactant by:
- Aincrease of temperature
- Bdecrease of temperature
- Cremoval of H2 from reaction mixture
- Daddition of Br2 into reaction mixture
92Which equation for equilibrium constant of reaction is correct N2 + 3 H2 <--> 2 NH3 :
- AK = [NH3]
-------------
[H2]³ . [N2] - BK = [NH3]²
-------------
[H2]³ . [N2] - CK = [N2] . [H2]
-------------
[NH3]² - DK = [N2] . [H2]³
- AK = [NH3]
93Which equation for equilibrium constant of reaction is correct 4KClO3 <--> KCl + 3 KClO4:
- AK = [KCl] . [KClO4]
-------------
[KClO3]4 - BK = [KCl] . [KClO4]²
----------------
[KClO3]³ - CK = [KClO3]4
---------------
[KCl] . [KClO4]³ - DK = [KCl] . [KClO4]³
-------------
[KClO3]4
- AK = [KCl] . [KClO4]
94Which equation for equilibrium constant of esterification is correct CH3OH + CH3COOH <--> CH3COOCH3 + H2O :
- AK = [CH3COOCH3] . [H2O]
- BK = [CH3COOCH3] . [H2O]
--------------------------------
[CH3OH] . [CH3COOH] - CK = [CH3OH] . [CH3COOH]
- DK = [CH3OH] . [CH3COOH]
--------------------------------
[CH3COOCH3] . [H2O]
95Which of following reactions express exothermic process:
- A2 SO3 --> 2SO2 + O2; Qm= +195 kJ.mol¹-
- BCO + 1 O2 --> CO2; Qm= -283 kJ.mol¹-
- C4 NH3 + 5 O2 --> 4 NO + 6 H2O; Qm= -906 kJ.mol¹-
- DN2 + 3H2 --> 2NH3; Qm= -93 kJ.mol¹-
96Activation energy of reaction:
- Aapplies only in exothermic reactions
- Bapplies in exothermic and endothermic chemical reactions
- Cis related to the rate of reaction
- Din influenced by presence of catalyst
97Which of following statements about reaction are correct 2NO² <--> N2O4; Qm= -57 kJ.mol¹- :
- Aby increase of temperature equilibrium state changes to the side of reactants
- Bin direction of N2O4 synthesis is endothermic
- Cby increase of temperature equilibrium state changes to the side of products
- Din direction of N2O4 synthesis is exothermic
98Which of following statements about reaction are correct 2 SO3 <--> 2 SO3 + O2; Qm= +195 kJ.mol¹-:
- Ain direction of SO3 synthesis is exothermic
- Bby decrease of temperature equilibrium state changes to the side of reactant
- Cby increase of temperature equilibrium state changes to the side of products
- Din direction of SO3 splitting is exothermic
99If reaction heat Qm in the reaction A + B ---> AB is positive, then:
- Aproduct of reaction is more stable than reactants
- Bduring reaction energy was spent
- Cvalue of activation energy is always high
- Dvalue of activation is always low
100Mark oxidation number of hydrogen in compounds:
- AI
- BI, VII
- C-I
- Donly I
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- Chemistry Quiz on Chemistry, created by Ana Caroline on 20/09/2017.
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