Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

BTEC Science > Mrs Ferrus - > Flashcards

Mrs Ferrus - Flashcards

1
Q

What is wavelength?

A

the difference between two points in phase on adjacent waves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is amplitude?

A

the maximum value of displacement in the oscillation cycle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is displacement?

A

is the distance moved by a wave or particle from its original position
it is also a vector

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is frequency?

A

it is the number of oscillations in one second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is a period?

A

is the time taken for each oscillation to pass a fixed point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the unit for wavelength?

A

metres, m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the unit for amplitude?

A

metres, m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the unit for frequency?

A

hertz, Hz

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q
A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the unit for period?

A

seconds, s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the equation that links frequency and period?

A

frequency = 1 / period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is wave speed?

A

is the speed at which energy is transferred through the medium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the wave equation?

A

wave speed = frequency x wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is electronegativity?

A

is the tendency of an atom to attract a bonding pair of electrons in a covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the first ionisation energy?

A

is the energy required to remove 1 mole of electrons from 1 mole of atoms in their gaseous state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why does the reactivity of halogens increase up the group?

A

because there is a smaller radius and less electron shielding which means a greater electrostatic attraction with the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the first ionisation energy equation?

A

X (g) —> X^+ (g) + e^-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is electron affinity?

A

is the energy released when 1 mole of gaseous atoms gain 1 mole of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the electron affinity equation?

A

X (g) + e^- —-> X^- (g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the reactivity series?

A

is the order of reactivity of metals

10
Q

What is the electromagnetic spectrum?

A

is the entire distribution of electromagnetic radiation according to frequency or wavelength

11
Q

What is the name given to group 1 of the periodic table?

A

alkali metals

12
Q

What is the electronic configuration of lithium?

A

1s2 2s1

13
Q

Write the equation to show the first ionisation energy of lithium?

A

Li (g) —> Li^+ + e^-

14
Q

A student burns magnesium in air to produce 1.40 g of magnesium oxide. The theoretical yield of magnesium oxide for the experiment is 2.00 g.
Calculate the percentage yield for the students experiment?

A

actual / theoretical x 100
1.40 / 2.00 x 100
= 70%

15
Q

Magnesium reacts with oxygen to form magnesium oxide.
2.43 g of magnesium was burned.
Calculate the theoretical yield of magnesium oxide.

A

RFM = 24.3 + 16 = 40.3
MOLE = 2.43 / 24.3 = 0.1
Mass of MgO = 0.1 x 40.3 = 4.03
= 4.03 g

16
Q

Calculate the mass of ammonia required to make 5.0 g of ammonium nitrate.
RFM of NH3 = 17
RFM of NH4NO3 = 80

A

mole of ammonium nitrate is 5 / 80 = 0.0625
mass of ammonia = 0.0625 x 17 = 1.0625
= 1.06 g

17
Q

Calculate the maximum mass of calcium chloride produced by reacting 8.02 grams of calcium with excess hydrochloric acid.
relative atomic mass: Ca = 40.1
relative atomic mass: CaCl2 = 111.1

A

mole of calcium is 8.02 / 40.1 = 0.2
mass of calcium chloride is 0.2 x 111.1 = 22.22
= 22.22 g

18
Q

Calculate the number of moles of hydrochloric acid in 50 cm2 of 0.2 M hydrochloric acid

A

converting 50 / 1000 - 0.05
0.05 x 0.2 = 0.01
= 0.01 moles

19
Q

A learner is given 6.02 g of magnesium sulfate. Calculate the number of moles of magnesium sulfate.
RFM of MgSO4 = 120.4

A

6.02 / 120.4 = 0.05
= 0.05

20
Q

The learner dissolves the magnesium sulfate in distilled water to make 500 cm3 of solution.
Calculate the molar concentration of this magnesium sulfate solution.
The number of moles is 0.05

A

conversion is 500 / 1000 = 0.5
0.05 / 0.5 = 0.1
= 0.1 mol dm3

21
Q

A sample of chlorine contains 80% chlorine-35 and 20% chlorine-37.
Chlorine the relative atomic mass of this sample of chlorine.

A

80 x 35 = 2800
20 x 37 = 740
2800 + 740= 3540
3540 / 100 = 35.4
= 35.4

22
Q

Calculate the relative formula mass for KMnO4

A

39.1 + 54.9 + (16 x 4 ) = 158
= 158

23
Q

Calculate the relative formula mass of ammonium chloride, NH4Cl

A

14.0 + ( 1.0 x 4 ) + 35.5 = 53.5
= 53.5

24
Q

Calculate the relative formula mass of iron oxide, Fe2O3

A

( 55.8 x 2 ) + ( 16.0 x 3 ) = 159.6
=159.6

25
Q

Calculate the relative formula mass for ethanol, C2H5OH

A

( 12.0 x 2 ) + ( 1.0 x 6 ) + 16 = 46
= 46

26
Q

Calculate the relative molecular mass for magnesium chloride, MgCl2

A

24.3 + ( 35.5 x 2 ) = 95.3
- 95.3

27
Q

What is the equation that shows the first ionisation of potassium?

A

K (g) —> K+ (g) + e-

28
Q

Complete the electronic configuration for a phosphorus atom

A

1s2, 2s2, 2p6, 3s2, 3p3

29
Q

Complete the electronic configuration for an atom of sodium

A

1s2, 2s2, 2p6, 3s1

30
Q

Magnesium reacts with sulfuric acid to form magnesium sulfate and hydrogen.
Complete the equation for this reaction.
___ + ____ —> MgSO4 + H2

A

Mg + H2SO4 —–> MgSO4 + H2

31
Q

Explain why the melting point increases as the atomic number increases

A

Higher atomic number means more electrons
More electrons mean temporary dipoles become larger
Intermolecular forces are stronger

32
Q

Complete the word equation for the reaction of calcium with sulfuric acid

A

Calcium + Sulfuric acid —–> Calcium sulfate + hydrogen

33
Q

Describe how a chlorine atom forms a chloride ion, Cl-

A

Chlorine atom gains one electron in outermost shell

34
Q

In an experiment, 4.6 g of sodium was reacted with chlorine.
The actual yield of the experiment was 7.5 g
Calculate the percentage yield
(relative formula mass of sodium chloride = 58.5)

A

moles of Na = 4.6 / 23 = 0.2
0.2 X 58.5 = 11.7
7.5 / 11.7 = 0.6
0.6 X 100 = 60
= 60%

35
Q

Describe the structure and bonding in aluminium metal

A

uniform layers in giant lattice
metallic bonding
sea of delocalised electrons
positively charged ions

36
Q

Describe the structure of an ionic compound

A

giant lattice
positive and negative ions
strong electrostatic attraction

37
Q

atomic radius l ionic radius
O = 0.073 l O2 = 0.140
F = 0.071 l F = 0.133
S = 0.102 l S2 = 0.185

Discuss the atomic radius and ionic radius data in table above

A

Fluorine and oxygen are in the same period
Fluorine has smaller atomic radius to oxygen
Sulfur and oxygen are in the same group
Sulfur has a larger atomic radius than oxygen and fluorine
because there is an extra shell of electrons
Ionic radius is lager than the atomic radius from the same element

38
Q

Explain how burning carbon in air can lead to the formation of carbon monoxide

A

Air contains oxygen
If oxygen is limited carbon monoxide forms

BTEC Science (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions