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Chemistry and Biology > General and Inorganic Chemistry > Flashcards

General and Inorganic Chemistry Flashcards

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1
Q

Elementary structural unit of the substance is:

a) proton
b) electron
c) atom
d) nucelon

A

c) atom

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2
Q

Proton is particle which:

a) has one elementary positive charge
b) has one elementary negative charge
c) does not belong among nucleons
d) belongs among nucleons

A

a) has one elementary positive charge

d) belongs among nucleons

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3
Q

The principal quantum number (n) describes:

a) The shape of the orbital
b) The orientation in space of the orbital
c) The orientation in space of a particular electron
d) The size of the orbital

A

d) The size of the orbital

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4
Q

Determine the values of the sub shell quantum number l, if n=3:

a) -1, 0, +1
b) 0, 1, 2
c) +1/2, -1/2
d) -2, -1, 0, +1, +2

A

b) 0, 1, 2

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5
Q

Ionic compounds:

a) majority of them are not soluble in water
b) majority of them are soluble in water
c) have the structure where cations and anions are attracted by electrostatic forces
d) as meltings or in solutions are conducting electric current

A

b) majority of them are soluble in water
c) have the structure where cations and anions are attracted by electrostatic forces
d) as meltings or in solutions are conducting electric current

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6
Q

In molecule of NH4CL among individual atoms there can be following bonds:

a) ionic
b) coordinate-covalent
c) covalent
d) hydrogen bond (H bond)

A

a) ionic
b) coordinate-covalent
c) covalent

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7
Q

Hydrogen bond:

a) is named hydrogen bridge
b) is stronger than covalent bond
c) is created between molecules (groups) which have atoms of hydrogen bound with strong electronegative elements (mainly F, O, N)
d) is responsible for the high boiling temperature of water

A

a) is named hydrogen bridge
c) is created between molecules (groups) which have atoms of hydrogen bound with strong electronegative elements (mainly F, O, N)
d) is responsible for the high boiling temperature of water

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8
Q

Van der Waal forces:

a) are created among anions and cations
b) are based on mutual effects of molecular dipoles
c) are 100 times weaker than covalent bond
d) are in complex compounds

A

b) are based on mutual effects of molecular dipoles

c) are 100 times weaker than covalent bond

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9
Q

Electronegativity 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:

a) covalent bond
b) Van-der-Waal forces
c) Coordinate-covalent
d) ionic bond

A

d) ionic bond

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10
Q

Sort by strength of listed bonds starting with strongest one:

a) ionic bond
b) hydrogen bond
c) covalent bond
d) Van-der-Waals force

A
  1. Covalent bond
  2. Ionic bond
  3. Hydrogen bond
  4. Van-der-Waals force
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11
Q

1 g of atomic hydrogen contains how many atoms:

a) 1,66606 x 10(-27)
b) 1 Mol
c) 6 x 10(23)
d) 1/12 u

A

b) 1 Mol

c) 6 x 10(23)

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12
Q

The molecular weight of glucose is 180. How many g of this substance is needed to generate 0.5 liters of a 2M (molar) solution?

a) 380g
b) 90g
c) 180g
d) 2 x 1,6606 x 10(-27) kg

A

c) 180g

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13
Q

A sample containing 0.0355 mol of salt with the formula XCl2 has a mass equal to 4.500g. Determine the X.

a) Mg
b) Fe
c) Zn
d) Ba

A

b) Fe

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14
Q

About the periodic table of elements it is true that:

a) atomic radius shrinks from left to right within a period
b) molecular weight increases from bottom to top
c) elements within a group have the same number of valence electrons
d) isotopes of every element are included

A

a) atomic radius shrinks from left to right within a period

c) elements within a group have the same number of valence electrons

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15
Q 
Allocate the listed elements towards their dedicated group: 
Calcium
Iodine
Neon
Potassium
A

Calcium - Alkaline earth metals
Iodine - halogen
Neon - noble gas
Potassium - Alkali metals

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16
Q

Nuclides 58Co27, 59Co27, 60Co27:

a) are isotopes
b) have the same number of protons
c) have the same number of neutrons
d) have different amount of nucleons

A

a) are isotopes
b) have the same number of protons
d) have different amount of nucleons

17
Q

Solution has acidic reaction if:

a) pH = 4,8
b) pOH = 11,9
c) pOH > 7
d) pH < 6

A

a) pH = 4,8
b) pOH = 11,9
c) pOH > 7
d) pH < 6

18
Q

Which equation for equilibrium constant of reaction is correct N2 + 3H2 2NH3:

a) K = [NH3] / ([H2]3) x [N2]
b) K = [N2] x ([H2]3) / ([NH3]2)
c) K = ([NH3]2) / ([H2]3) x [N2]
d) K = [N2] x ([H2]3)

A

c) K = ([NH3]2) / ([H2]3) x [N2]

! Nicht auf c) achten ! Im Skript gibt es kein a), b), c), d)

19
Q

pOH of solution is 12. What is concentration of hydroxide and protons ions:

a) c(OH-) = 1 x 10(-12) mol/l
b) c(OH-) = 1 x 10(-2) mol/l
c) c(H+) = 1 x 10(-12) mol/l
d) c(H+) = 1 x 10(-2) mol/l

A

a) c(OH-) = 1 x 10(-12) mol/l

d) c(H+) = 1 x 10(-2) mol/l

20
Q

How much NaOH is present in 5 litres of solution pH of which is 12? Mr(NaOH) = 40:

a) 20g
b) 0,4g
c) 2g
d) 400mg

A

c) 2g

21
Q

There are two solutions. Solution A with value of pOH = 10 and solution B with value pOH = 12. About these solutions we may say:

a) solution A is more acidic than solution B
b) pH of solution B is lower than pH of solution A
c) pH of solution A is bigger by 2 than pH of solution B
d) in solution A concentration of H3O+ ions is 100 times bigger than in solution B

A

b) pH of solution B is lower than pH of solution A

c) pH of solution A is bigger by 2 than pH of solution B

22
Q

Which of following hydroxides completely neutralize 0.4 mol of ocalic acid:

a) 0.6 mol NaOH
b) 0.4 mol Ba(OH)2
c) 0.8 mol LiOH
d) 0.4 mol Mn(OH)2

A

b) 0.4 mol Ba(OH)2
c) 0.8 mol LiOH
d) 0.4 mol Mn(OH)2

23
Q

What is the pH value of a 0.42M sodium hydroxide solution at 25°C?

a) 0.38
b) 13.58
c) 13.62
d) 0.42

A

c) 13.62

24
Q

Calculate the amount of sulphuric acid in 2.500 cm3 of solution with concentration 0.6 mol.dm-3. Mr(H2SO4) = 98:

a) 15 mol
b) 12 mol
c) 1.5 mol
d) 0.147 kg

A

c) 1.5 mol

d) 0.147 kg

25
Q

Calculate the amount of SO2 which is formed by burning of 112 grams of sulphur and the amount of oxygen required for the reaction. Ar(S) = 32; Ar(O)=16: S+O2 –> SO2

a) 112g O2
b) 7 mol O2
c) 78.4 dm3 SO2
d) 3.5mol O2

A

a) 112g O2
c) 78.4 dm3 SO2
d) 3.5mol O2

26
Q

Calculate the amount of zinc and sulphur required for preparation of 24.25 g zinc sulphide (ZnS). Ar(Zn) = 65; Ar(S) = 32:

a) 0.25 mol of S
b) 0.50 mol of Zn
c) 16.25g of S
d) 0.20 mol of Zn

A

a) 0.25 mol of S

27
Q

Reduction:

a) is every chemical reaction during which either atoms of ions of elements accept electrons
b) is every chemical reaction during which either atoms of ions of elements lose electrons
c) is the process during which positive oxidation number of atoms decreases
d) is the process during which positive oxidation number of atoms increases

A

a) is every chemical reaction during which either atoms of ions of elements accept electrons
c) is the process during which positive oxidation number of atoms decrease

28
Q

Iodine atom has oxidation number VII in compounds:

a) NaIO
b) I2O7
c) PbI2
d) NH4I

A

b) I2O7

29
Q

Atoms, ions, and molecules characterized by a large affinity for electrons tend to be good:

a) Oxidizing agents
b) Reducing agents
c) Electrolytes
d) Bases

A

a) Oxidizing agents

30
Q

In a given redox reaction the oxidation
number of phosphorus changes from -3 to 0. This means:
a) Loss of three electrons and thus reduction of P.
b) Loss of three electrons and thus oxidation of P.
c) Gain of three electrons and thus reduction of P.
d) Gain of three electrons and thus oxidation of P.

A

b) Loss of three electrons and thus oxidation of P.

31
Q

Which of following reactions express exothermic process:
a) 2SO3 –> 2SO4 + O2; Qm = +195 kJ.mol-1

b) CO + l O2 –> CO2; Qm = -283 kJ.mol-1
c) 4NH3 + 5O2 –> 4NO + 6H2O; Qm = -906 kJ.mol-1
d) N2 + 3H2 –> 2NH3; Qm = -93 kJ.mol-1

A

b) CO + l O2 –> CO2; Qm = -283 kJ.mol-1
c) 4NH3 + 5O2 –> 4NO + 6H2O; Qm = -906 kJ.mol-1
d) N2 + 3H2 –> 2NH3; Qm = -93 kJ.mol-1

32
Q

Which of following statements about reaction are correct
2SO3 2SO2 + O2; Qm = -195 kJ.mol-1:

a) In direction of SO3 synthesis is exothermic
b) By decrease of temperature equilibrium state changes to the side of reactant
c) By increase of temperature equilibrium state changes to the side of products
d) In direction of SO3, splitting is exothermic

A

a) In direction of SO3 synthesis is exothermic
b) By decrease of temperature equilibrium state changes to the side of reactant
c) By increase of temperature equilibrium state changes to the side of products

33
Q

Equilibrium state of the reaction:

a) is the state when reaction proceeds at the same rate in both directions
b) is the state when reactants are completely changed to products
c) is expressed by equilibrium constant
d) is the state when concentrations of reactants in reaction mixture are the same as concentrations of products

A

a) is the state when reaction proceeds at the same rate in both directions
c) is expressed by equilibrium constant

34
Q

There is a graph that shows an Energy diagram of chemical reaction, which shows a graph with two hills. The beginning is on a higher energy level than the end of the graph.
It represents:

a) Endergonic reaction
b) Exergonic reaction
c) Catalysis
d) Condensation reaction

A

b) Exergonic reaction

c) Catalysis

35
Q

Which of these factors will not speed up a chemical reaction?

a) Increase of the temperature
b) Increase of the particle size of reactants
c) Increase of the reactants concentrations
d) Addition of a catalyst

A

b) Increase of the particle size of reactants

36
Q

Given is the equation of the chemical reaction: MnO4- + 8 H3O + 5 Fe2+ –> 5 Fe3+ + Mn2+ + _???_H2O What is the proper coefficient in front of H2O?

a) 4
b) 8
c) 12
d) 16

A

c) 12

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