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Science > Gr.11 T2 Chemistry > Flashcards

Gr.11 T2 Chemistry Flashcards

1
Q

What are valence electrons?

A

The number of electrons in the outermost energy level of an atom.

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2
Q

What is electrostatic force?

A

The force of attraction or repulsion between two charged particles.

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3
Q

What are chemical bonds?

A

The net electrostatic force that two atoms sharing electrons exert on each other.

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4
Q

What is potential energy?

A

Energy due to the position of objects

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5
Q

What is the main reason for atoms to bond?

A

Increased stability due to lower potential energy

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6
Q

What is a dative covalent bond?

A

A bond where both electrons in the shared pair belong to the same atom.

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7
Q

What is the VSEPR-theory?

A

Valence electron pairs will repel each other so that they are as far from each other as possible.

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8
Q

Give examples of electron regions

A

Lone pair
Shared pair of electrons
Double/ triple bonds = 1 electron region
Etc.

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9
Q

What is the shape of a molecule with 2 electron regions without lone pairs?
Also state the bond angle.

A

Linear

Bond angle = 180 degrees

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10
Q

What is the shape of a molecule with 3 electron regions without lone pairs?
Also state the bond angle.

A

Trigonal planar

Bond angle = 120 degrees

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11
Q

What is the shape of a molecule with 4 electron regions without lone pairs?
Also state the bond angle.

A

Tetrahedral

Bond angle = 109,5 degrees

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12
Q

What is the shape of a molecule with 5 electron regions without lone pairs?
Also state the bond angle.

A

Trigonal bipyramidal

Bond angle = 120 degrees in trigonal plane and 90 degrees between plane and top and bottom atoms

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13
Q

What is the shape of a molecule with 6 electron regions without lone pairs?
Also state the bond angle.

A

Octahedral

Bond angle = 90 degrees

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14
Q

What is the shape of a molecule with 4 electron regions with 2 lone pairs?
Also state the bond angle. 💧

A

Angular

Bond angle = 104,5 degrees

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15
Q

What is the shape of a molecule with 4 electron regions with 1 lone pair?
Also state the bond angle.

A

Trigonal pyramidal

Bond angle = 109 degrees

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16
Q

What is electronegativity?

A

The tendency of an atom to attract electrons towards itself and form a negative ion.

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17
Q

Below what point is a bond with a difference in EN a polar covalent bond?

A

< 2,1

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18
Q

What will be zero if a molecule is non-polar?

A

The net dipole moment is 0

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19
Q

What will be zero if a bond is non-polar?

A

The difference in electronegativity between the atoms

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20
Q

What is another name for a non-polar molecule?

A

A symmetrical molecule

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21
Q

What is a bond?

A

An electrostatic force of attraction holding atoms together.

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22
Q

What is bond energy?

A

The energy needed to break a bond in a molecule when reagents are in the gas phase at standard conditions.

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23
Q

What is bond length?

A

The average distance between the nuclei of two bonded atoms.

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24
Q

What are forces between molecules called?

A

Intermolecular forces

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25
Q

What are forces that hold atoms together inside a molecule called?

A

Intramolecular forces

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26
Q

What are the 5 types of intermolecular forces?

A 
Ion-dipole forces
Ion-induced-dipole forces
Dipole-dipole forces (some of which have hydrogen bonding)
Dipole-induced-dipole forces
London forces
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27
Q

When are dipole-dipole forces hydrogen bonding?

A

When they are between a hydrogen atom covalently bonded to N,O or F and N,O or F of a neighbouring molecule.

28
Q

Why is hydrogen bonding so strong?

A

N,F,O have high electronegativity. Hydrogen atom left with no electrons (very positive).
Therefore a very strong dipole.

Valence electrons of N,F,O in second energy level (small atoms). Overall, molecules are small. Can get close to each other.
Therefore a stronger dipole-dipole force.

29
Q

What is a melting point?

A

The temperature at which a solid becomes a liquid.

30
Q

What is the relationship between the molecular mass and the intermolecular forces of a substance?

A

Bigger molecular mass = stronger intermolecular forces

31
Q

What is the relationship between the density and the intermolecular forces of a substance?

A

Higher density = stronger intermolecular forces

32
Q

What is thermal expansion?

A

The ability of a substance to expand (increase in volume) with an increase in temperature

33
Q

What is thermal conductivity?

A

A material’s ability to conduct heat energy.

34
Q

What is the relationship between thermal conductivity and the intermolecular forces of a substance?

A

Stronger IMF = better thermal conductivity

35
Q

Why do metals have high thermal conductivity?

A

Atoms are held together in a crystal lattice by strong electrostatic forces. Vibrations are passed on easily because particles are packed closely together.

36
Q

What is viscosity?

A

The resistance of a liquid to flow.

37
Q

What is the relationship between viscosity and the intermolecular forces of a substance?

A

Stronger IMF = more viscous liquid

38
Q

What are adhesion forces?

A

Forces between molecules of a substance and sides of the container.

39
Q

What are cohesion forces?

A

Forces between the molecules of a substance.

40
Q

Define specific heat capacity

A

The amount of heat required to raise the temperature of 1g of a substance with 1*C

41
Q

What do you call it when a liquid can flow in narrow spaces without assistance of external forces?

A

Capillary action

42
Q

What is molar mass?

A

The mass of one mol of a substance.

43
Q

How many kelvin is 0*C?

A

273K

44
Q

3

What is 1 litre in dm ?

A

3

1 dm

45
Q

What is a bond angle?

Double-check with someone

A

The angle between atoms bonded to a central atom.

46
Q

What is 1 atm in Pa?

A

5

1 atm = 1,013 x 10 Pa

47
Q

Give the unit for each variable in the formula:

     V n = -----
    Vm
A

n - mol
3
V / Vm (22,4) - dm

48
Q

What is the standard temperature and pressure (STP)?

A

Temperature: 0*C (273K)

                            5 Pressure: 1,013x10  Pa (1 atm)
49
Q

Give the unit for each variable in the formula:

pV=nRT

A 
p - Pa
V - m3
n - mol
R - gas constant (8,31)
T - K
50
Q

What does a solution consist of?

A

Solute (solid) dissolved in a solvent (liquid)

->homogeneous mixture

51
Q

What is molar concentration?

A

The amount of solute in moles per volume of solution.

52
Q

Give the unit for each variable in the formula:

     n c = ----
     V
A

-3
c - mol.dm (molar concentration)
n - mol
V - dm3

53
Q

Give another version of this formula:

     n c = ----
     V
A

m
c = ——
MV

54
Q

What do square brackets show?

A

Concentration of the substance

55
Q

What is a standard solution?

A

A solution where the molar concentration is known precisely

56
Q

How is a standard solution made?

Make the solvent water for this example

A

Calculate how many grams of the solute you will need.
Measure out that mass by putting small amounts of it into a watch glass on a scale until you reach that mass.
Empty it through a funnel into a volumetric flask.
Rinse the last bit from the watch glass and funnel using distilled water.
Add a bit more distilled water and swirl the contents until the solute has dissolved.
Fill the volumetric flask up to the line with distilled water.

57
Q

What is a limiting reactant?

A

The reactant that limits the amount of product formed.

58
Q

How do you calculate percentage yield?

A

Actual yield
—————– x 100
Theoretical yield

59
Q

Give the formula for stomach acid

A

HCl

60
Q

What unit is used for actual/ theoretical yield?

A

g

61
Q

How do you calculate percentage purity?

A

mass of pure compound
————————- x100
mass of total sample

62
Q

What is a bond angle?

A

The angle between two atoms bonded to a central atom.

63
Q

What unit is sometimes replaced with by “M” (for molarity)?

A
  • 3
    mol. dm

(The unit for molar concentration)

64
Q

When asked to give mole quantity or amount, answer is x mol.

When asked to give the number of ions/ molecules etc., multiply mole quantity by Avogadro’s number.

A

🌺

65
Q

Ionic bond

A

A chemical bond between a metal and a non-metal where electrons are transferred.

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