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KME Chemistry > 4 Sem, 1 Exam > Flashcards

4 Sem, 1 Exam Flashcards

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1
Q

What particles do the three states of matter have?

Solid, liquid, gas

A

localized particles, movable particles, independent particles

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2
Q

Density of g,l,s?

A

low, high, high

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3
Q

Volume of g,l,s?

A

indefinite, definite, definite

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4
Q

Shape of g,l,s?

A

indefinite, indefinite, definite

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5
Q

Distance between single units g,l,s and there freedom?

A

far away/independent, close together/mobile, close together fixed

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6
Q

IMF between g,l,s?

A

weak, moderate, strong

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7
Q

Unsymmetrical distribution of electrons in atom/molecule shells i.e. more electrons are on one side than the other which results in a charge. What are these charges/forces and the charged areas of the atom called?

A

Van der Waals forces (VdW-forces) a.k.a. London forces

Polarisation, temporary/instantaneous dipole

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8
Q

A positive dipole attracts the electrons of a neighboring atom/molecule towards itself causing a polarization in the other atom/molecule.

A

Induction of a dipole

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9
Q

What is the hierarchy of the IMF? Highest to lowest strength.

A
  1. Hydrogen bonds
  2. Dipole-dipole forces
  3. Van der Waals forces
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10
Q

With what do the Van der Waals forces increase?

A

With the probability of polarization i.e. the more electrons contained in a molecule. In the case of an equal number of electrons the size of the atom/molecule is important i.e. the larger the molecule/atom the more VdW-forces.

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11
Q

What does a high boiling point imply?

A

High intermolecular forces between the atoms/molecules

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12
Q

In a molecule out of more than one different atoms the different atoms must have a different amount of protons. The atom with more protons has a greater attraction on the electrons than the ones with less electrons forming a permanent dipole. These charges decrease rapidly with the size of the atom so that this effect decreases further down the periodic table. What is this combined effect called/its unit of measurement?

A

Electronegativity (ΔEN)

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13
Q

The atoms in a molecule with a higher electronegativity attract more electrons and therefore create permanent dipoles. What are the forces acting between such molecules called?

A

Dipole-dipole force or dipole-dipole interaction

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14
Q

Which element has the highest electronegativity?

A

Fluorine

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15
Q

What is the result of a difference in electronegativity of atoms in a molecule?
And what is the result of a increasing difference?

A

polar covalent bonds

increase in polarity

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16
Q

In what case can a molecule with polar bonds/a polar bond not have a dipole?

A

When the centers of the negative and positive dipole collide / are located at the same place.

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17
Q

What is necessary for the formation of a dipole? (2)

A 
Molecule contains (a) polar bond(s) (ΔEN)
the negative and positive dipole centers don't coincide
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18
Q

Because molecules containing hydrogen atoms directly bonded to fluorine, oxygen or nitrogen have a very large electronegativity difference, due to the hydrogens single proton and the small size of these atoms, they have particularly strong dipole-dipole forces and are assigned an own IMF. What is it called?

A

Hydrogen bonding

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19
Q

Because of hydrogen bonds water shows strange properties called the anomaly of water. What are these properties?

A

Denser liquid state than solid state

Water is most dense at 4°C

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20
Q

Why does H2O increase when it freezes?

A

In the solid state the molecules try to make as many H-bonds as possible. In the ideal orientation each molecule makes 4 hydrogen bonds leaving “tunnels” between the molecules.

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21
Q

What other physical factor (besides temperature) turns ice to water?
Why?
Name a real world application.

A

Pressure
Molecules are forced out of their arrangements into the “tunnels”
Ice-skating

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22
Q

Why do oil and water not mix?

A

Because polar (water) and non-polar (oil) substances don’t mix. Polar substances have a dipole, non-polar don’t.

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23
Q

How does a metal with x electrons on its outer shell interact with a nonmetal which has “n(max. shell) – x” electrons in its outer shell? What do the two atoms become?

A

The metal hands over its electrons to the non metal, both then achieving the noble gas state. Both become charged ions (metal +, nonmetal -)

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24
Q

What is a positive and a negative ion called?

A

cation (+), anion (-)

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25
Q

What is a salt?

A

Cations and anions attracting one another by strong Coulomb forces arranged in a periodical lattice.

26
Q

Pronounce NaCl.

A

sodium chloride

27
Q

What is the difference in structure between molecules and salts?

A

Salts do not have a limited or finite structure/lattice.

28
Q

__________ are substances which are composed of two different elements, one being a nonmetal and the other a metal.

A

Binary ionic compounds

29
Q

How do you name a binary ionic compound?

A

The metal is named first followed by the nonmetal with “-ide” (e.g. oxide, chloride)

30
Q

Can a salt be charged?

A

no

31
Q

Which elements are able to build several, different charged ions? And how are the these ions written?

A

Transition metals (d-block)
With roman numerals in brackets after the element name.
E.g. Fe^3+ => iron(III) ion

32
Q

What are ions out of one atom and ions out of many atoms called?

A

single atomic ions

polyatomic ions

33
Q

Many acids can easily be turned into polyatomic ions, how?

A

By separating a proton (1 H^+ ion)

34
Q

Anions and cations have very strong attracting forces. What does this result in?

A

Ionic bonds, the many attracting ions group around eachother and form a lattice structure

35
Q

What happens energy-wise when ions form a lattice structure? Exothermic or endothermic?

A

lattice energy or lattice enthalpy is released

=> exothermic

36
Q

In which two ways can the lattice energy of salts be measured/deduced?

A

melting points, ionic charges (+1/-1, +2/-2…..)/anion radius (decreases)

37
Q

What are salt melting points proportional to?

A

The lattice energy in the salts, this energy has to be put back in to break the structure and melt the salts

38
Q

The phenomenon that happens in the case of a movement or flow of electric charges?

A

electricity

39
Q

Which conduct electricity: salt solutions, solid salts, molten salts?

A

yes, no, yes

40
Q

When do substances conduct electricity?

Why do metals conduct electricity?

A

When there are movable charged particles

Because of there movable electrons

41
Q

What happens to ions when dissolved in water?

A

They are surrounded by water molecules, + H2O dipole to anions, - H2O dipole to cations

42
Q

How do you show in a chemical equation that a ion is dissolved in water?

A

small (aq) for (aqua) bottom left of atomic symbol.

43
Q

The electrical conductivity of salt solutions and molten salts is based on the migration of movable ions within an electric field. Say the electric field is produced by two electrodes. What are the positive and negative electrodes called?

A

anode (+ pole), cathode (- pole)

44
Q

What happens once ions have reached the respective electrode?

A

They are discharged

45
Q

There are two classes of conductors. The substances of the 1st class conduct electricity because of freely moving electrons and do not change during conduction. The substances of the 2nd class conduct electricity by the migration of ions and change chemically during conduction. What are these classes called?

A
  1. metals (and graphite)

2. electrolytes (=liquid conductors)

46
Q

What is the deposition of a discharged ion called?

A

precipitation

47
Q

Is the formation of a solvation shell an exothermic or endothermic reaction?

A

exothermic

48
Q

What does the fact that some salts dissolve in an exothermic reaction and others in an endothermic one depend on?

A

The size of the two reactions:
The endothermic destruction of the lattice structure, and,
The exothermic creation of a solvation shell

49
Q

Give the equation (math. and lang.) for the dissolution energy depending on the destruction of the lattice structure and the creation of a solvation shell in salts.

A

ΔH (dissolution) = ΔH (solvation) + ΔH (lattice)

enthalpy of solution / of dissolution = lattice energy + enthalpy of solvation

50
Q

How do dissolved ions and water molecules interact?

A

Ions are surrounded by water molecules.
Cations are surrounded by the negatively charged pole on the oxygen side and the anions by the positively charged hydrogen sides.

51
Q

If there are two electrodes with opposite charges in a salt solution, to which electrode will (a) the anions and (b) the cations migrate?

A

a) anode

b) cathode

52
Q

Why does ice decrease in a glass of ice-water if mixed with salt?

A

1st ions being released from a salt lattice structure is an endothermic reaction
2nd then the water molecules forming a solvation shell around the ions in an exothermic reaction

53
Q

When a salt and water make a salt solution what is the dissolution and what the solvation?

A 
solvation = solvation shell created around the ions
dissolution = the whole process of salt being dissolved
54
Q

What is the chemical formula of sulphuric acid and what are its polyatomic anions?

A

H2SO4
hydrogen sulphate : HSO4^-
sulphate : SO4^2-

55
Q

What is the chemical formula of carbonic acid and what are its polyatomic anions?

A

H2CO3
hydrogen carbonate: HCO3^-
carbonate: CO3^2-

56
Q

What is the chemical formula of phosphoric acid and what are its polyatomic anions?

A

H3PO4
dihydrogen phosphate: H2PO4^-
hydrogen phosphate: HPO4^2-
phosphate: PO4^3-

57
Q

What is the chemical formula of nitric acid and what are its polyatomic anions?

A

HNO3

nitrate: NO3^-

58
Q

What is the chemical formula of acetic acid and what are its polyatomic anions?

A

CH3COOH

acetate: CH3COO^-

59
Q

What is the chemical formula of chloric acid and what are its polyatomic anions?

A

HClO3

chlorate: ClO3^-

60
Q

What is the chemical formula of water and what are its polyatomic anions?

A

H2O

hydroxide: OH^-

61
Q

Name the formula for these two polyatomic cations: ammonium ions and hydronium ions.

A

NH4^+

H3O^+

KME Chemistry (5 decks)

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