KERBOODLE SUMMARY QUESTIONS: EL COPY Flashcards by hubooshi Abduljhbar

Q

Complete the table

A

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Q

State the number of protons, neutrons, and electrons present in

A

35 protons
44 neutrons
35 electrons

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Q

State the number of protons, neutrons, and electrons present in

A

35 protons
46 neutrons
35 electrons

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Q

State the number of protons, neutrons, and electrons present in

A

17 protons
18 neutrons
17 electrons

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Q

State the number of protons, neutrons, and electrons present in

A

17 protons
20 neutrons
17 electrons

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Q

Using the isotopes and their abundances, work out the relative atomic mass of bromine

A

A_r of Br = 80.0

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Q

Using the isotopes and their abundances, work out the relative atomic mass of bromine

A

A_r of Ca = 40.1

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Q

The relative atomic mass of the element iridium is 192.2. Iridium occurs naturally as a mixture of iridium-191 and iridium-193.

Calculate the percentage of each isotope in naturally occuring iridium if the value for the relative atomic mass is taken to be 192.2

A

take iridium-193 to be x%
iridium-191 = 100-x%
193x and 191(100-x)
(193x+19100-191x)/100 = 192.2
2x+19100=19220
2x=19220-19100
2x=120
x=60

iridium-193 = 60%
iridium-191 = 40%

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Q

Write a nuclear equation for a ⁷Li nucleus that absorbs a colliding proton and then disintegrates into two identical fragments

A

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Q

Write a nuclear equation for the production of carbon-14 by collision of a neutron with an atom of nitrogen-14

A

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Q

The relative atomic mass of antimony is 121.8. Antimony exists as two isotopes - antimony-121 and antimony-123.

Calculate the relative abundances of the two isotopes

A

antimony-123 = 40%
antimony-121 = 60%

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Q

Lithium carbonate is used to give the bright red colour to a firework. The visible region of the emission spectrum of lithium contains several coloured lines with a particularly intense line at the red end of the spectrum. The emission spectrum is shown below

Which line, green or red, has a greater frequency?

A

green

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for Li⁺?

A

bright red

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for Na⁺?

A

orange

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for K⁺?

A

lilac

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for Ca²⁺?

A

brick red

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for Ba²⁺?

A

apple green

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Q

Flame tests can be used to identify some metal cations.

What is the flame colour for Cu²⁺?

A

blue-green

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Q

Describe the similarites and differences between an emission spectrum of lithium and an absorption spectrum of lithium

A

Similarities: line spectrum; lines in the same place because have same frequencies
lines get closer together with increasing frequency

Differences: black lines on a bright coloured continuous spectrum background for absorption spectrum

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Q

Draw an energy level diagram with two arrows. One to represent an electron energy level change that might give rise to the red line and the other to represent an energy level change that might give rise to the green line.

A

both arrows pointing downwards
shorter arrow represents red line
longer arrow represents gree line

both arrows must start and finish on lines; does not matter which levels they go between

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Q

Calculate the frequency of electromagnetic radiation with a wavelength of 5.5 x 10^-7m

A

5.5 x 10¹⁴ s^-1

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Q

1s² is an example of a notation for electronic configuration

What does the number 1 refer to?

A

The electrons are in the first electron shell

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Q

1s² is an example of a notation for electronic configuration

What does the s refer to?

A

The electrons are in an s type orbital

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Q

1s² is an example of a notation for electronic configuration

What does the superscript 2 refer to?

A

There are two electrons in this orbital

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Write out the electronic configuration for boron (Z=5)

1s²2s²2p¹

Write out the electronic configuration for phosphorus (Z=15)

1s²2s²2p⁶3s²3p³

The electronic configuration of the outermost shell of an atom of an element X is 3s²3p⁴ What is the atomic number and name of the element

Z=16 element is sulfur

Electronic configurations are sometimes abbreviated by labelling the core of filled inner shells as the electronic configuration of the appropriate noble gas. Name the element from the electronic configuration [Ne] 3s²3p⁵

chlorine

Electronic configurations are sometimes abbreviated by labelling the core of filled inner shells as the electronic configuration of the appropriate noble gas. Name the element from the electronic configuration [Ar] 4s¹

potassium

Electronic configurations are sometimes abbreviated by labelling the core of filled inner shells as the electronic configuration of the appropriate noble gas. Name the element from the electronic configuration [Ar] 3d²4s²

titanium

Electronic configurations are sometimes abbreviated by labelling the core of filled inner shells as the electronic configuration of the appropriate noble gas. Name the element from the electronic configuration [Kr] 4d¹⁰5s²5p²

tin

The electron shell configuration for sodium can be written as 2.8.1. Use this notation to write down the electron configuration for lithium

2.1

The electron shell configuration for sodium can be written as 2.8.1. Use this notation to write down the electron configuration for phosphorus

2.8.5

The electron shell configuration for sodium can be written as 2.8.1. Use this notation to write down the electron configuration for calcium

2.8.8.2

The electron shell configurations of unknown elements A to E are given below. Which of these elements are in the same group? ## Footnote **A)** 2.8.2 **B)** 2.6 **C)** 2.8.8.2 **D)** 2.7 **E)** 2.2

A, C and E

Complete the table below

Classify the element [Kr] 5s¹ as a s-, p-, d-, or f-block element

s-block

Classify the element 1s²2s²2p⁶3s²3p⁴ as a s-, p-, d-, or f-block element

p-block

Classify the element [Ar] 3d¹⁰4s²4p⁶ as a s-, p-, d-, or f-block element

p-block

Classify the element [Xe] 6s²as a s-, p-, d-, or f-block element

s-block

Classify chromium as a s-, p-, d-, or f-block element

d-block

Classify aluminium as a s-, p-, d-, or f-block element

p-block

Classify uranium as a s-, p-, d-, or f-block element

f-block

Classify strontium as a s-, p-, d-, or f-block element

s-block

Draw an electron dot-and-cross diagram for chlorine, Cl₂

Draw an electron dot-and-cross diagram for hydrogen chloride, HCl

Draw an electron dot-and-cross diagram for methane, CH₄

Draw an electron dot-and-cross diagram for hydrogen sulfide, H₂S

Draw an electron dot-and-cross diagram for aluminium bromide, AlBr₃

Draw an electron dot-and-cross diagram for silicon chloride, SiCl₄

Draw an electron dot-and-cross for ethene

Draw an electron dot-and-cross for ethyne

Draw an electron dot-and-cross for methanol

Ammonia, NH₃, and boron trifluoride, BF₃, combine together to form the molecule NH₃BF₃ This molecule has a dative covalent bond between the nitrogen atom and the boron atom Draw a dot-and-cross diagram for this molecule

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in SiH₄. Give the bond angles you would expect.

109.5

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in H₂S. Give the bond angles you would expect.

104.5

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in PH₃. Give the bond angles you would expect.

107

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in CO₂. Give the bond angles you would expect.

180

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in SF₂. Give the bond angles you would expect.

104.5

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in BCl₃. Give the bond angles you would expect.

120

Draw an electron dot-and-cross diagram to show the bonding pairs and lone pairs of electrons in C₂H₂. Give the bond angles you would expect.

180

Draw a diagram to show the bonds and lone pairs of electrons in CH₃CH₃. Give the bond angles you would expect.

109.5

Draw a diagram to show the bonds and lone pairs of electrons in CH₃OH. Give the bond angles you would expect.

Draw a diagram to show the bonds and lone pairs of electrons in CH₃NH₂. Give the bond angles you would expect.

Draw a diagram to show the bonds and lone pairs of electrons in CH₂=CH₂. Give the bond angles you would expect.

120

Draw a diagram to show the bonds and lone pairs of electrons in CH₃C≡N. Give the bond angles you would expect.

Draw a diagram to show the bonds and lone pairs of electrons in NH₂OH. Give the bond angles you would expect.

no answer in textbook = ask miss

Draw a diagram to show the bonds and lone pairs of electrons in COCl₂. Give the bond angles you would expect.

textbook doesnt give an answer = ask miss

What shape is NF₃?

pyramidal

What shape is BF₃?

trigonal planar

What shape is SF₆?

octahedral

One atom of element X is approximately 12 times heavier than one carbon atom. What is the approximate relative atomic mass of this element? Hence identify X.

relative atomic mass = 144 neodymium, Nd

Balance the equation: Mg + O₂ --\> MgO

2Mg + O₂ --\> 2MgO

Balance the equation: H₂ + O₂ --\> H₂O

2H₂ + O₂ --\> 2H₂O

Balance the equation: CaCO₃ + HCl --\> CaCl₂ + CO₂ + H₂O

CaCO₃ + 2HCl --\> CaCl₂ + CO₂ + H₂O

Balance the equation: HCl + Ca(OH)₂ --\> CaCl₂ + H₂O

2HCl + Ca(OH)₂ --\> CaCl₂ + 2H₂O

Balance the equation: CH₃OH + O₂ --\> CO₂ + H₂O

2CH₃OH + 3O₂ --\> 2CO₂ + 4H₂O

Write a balanced equation including state symbols for zinc reaction with sulfuric acid to form zinc sulfate and hydrogen.

Zn_(s) + H₂SO_4(aq) --\> ZnSO₄_(aq) + H_2(g)

Write a balanced equation including state symbols for magnesium carbonate, MgCO₃, decomposing on heating to form magnesium oxide and carbon dioxide

MgCO_3(s) --\> MgO_(s) + CO_2(g)

Write a balanced equation including state symbols for barium oxide reacting with hydrochloric acid to form barium chloride and water.

BaO_(s) + 2HCl_(aq) --\> BaCl_2(aq) + H₂O_(l)

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) Why do we need to know the mass of the sample as well as the masses of the elements in it?

The mass of the sample is needed to be sure that iodine and oxygen are the only elements in the compound

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) In step 2, what do the numbers 0.1 and 0.25 represent?

The relative number of moles of iodine and oxygen

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) Why, in step 3, do we divide both 0.1 and 0.25 by 0.1?

To change the relative number of moles into the ratio of moles of oxygen relative to 1 mole of iodine

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) Why have we doubled the numbers in moving from step 3 to 4?

In order to produce a ratio involving whole numbers

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) Write down three possibilities for the molecular formula of this compound based on its empirical formula

I₂O₅, I₄O₁₀, I₆O₁₅ etc.

The empirical formula of a compound can be calculated when you know the masses of the elements in a sample of it. The steps to calculate the empirical formula of a compound if a 16.7g sample of it contains 12.7g of iodine and 4.0g of oxygen is shown below (Units have been omitted) What additional information do you need to work out the actual molecular formula of the compound?

The molar mass is needed

How many moles of atoms are in 32.1g of sulfur?

1 mole

How many moles of atoms are in 31.8g of copper?

0.5 moles

Why would the moles of atoms in a sample of 32.1g of sulfur be different to the moles in a sample of 32.1g of copper?

Atoms of copper are approximately twice as heavy as atoms of sulphur Thus around the same mass would contain only half as many moles of copper as it does of sulfur

How many moles are there in 88g of carbon dioxide?

2 moles

How many moles are there in 2.92g of sulfur hexafluoride, SF₆?

0.02 moles

How many moles are there in 0.37kg of calcium hydroxide, Ca(OH)₂?

5 moles

How many moles are there in 18 tonnes of water (1 tonne = 1 x 10⁶g)?

1.0 x 10⁶ moles

Draw an ionic dot-and-cross diagram for lithium hydride, LiH

Draw an ionic dot-and-cross diagram for potassium fluoride, KF

Draw an ionic dot-and-cross diagram for magnesium oxide, MgO

Draw an ionic dot-and-cross diagram for calcium sulfide, CaS

Which type of structure would you expect a white solid which starts to soften at 200^oC and can be drawn into fibres to have?

macromolecular (covalent molecular)

Which type of structure would you expect a white solid which melts at -190^oC to have?

simple molecular (covalent molecular)

Which type of structure would you expect a white solid which melts at 770^oC and conducts electricity when molten, but not in the solid state

ionic (giant lattice)

Draw an ionic electron dot-and-cross for calcium chloride, CaCl₂

Draw an ionic electron dot-and-cross for sodium sulfide, Na₂S

An ammonia molecule, NH₃, forms a dative bond with hydrogen ion, H⁺, to produce an ammonium ion, NH₄⁺. The other three hydrogen atoms are held to the nitrogen atom by conventional covalent bonds. What is the essential difference between a dative bond and a covalent bond?

In a normal covalent bond, each atom supplies a single electron to make up the pair of electrons involved in the bond. In a dative covalent bond one atom supplies both electrons.

An ammonia molecule, NH₃, forms a dative bond with hydrogen ion, H+, to produce an ammonium ion, NH₄⁺. The other three hydrogen atoms are held to the nitrogen atom by conventional covalent bonds. Draw a dot-and-cross diagram for the ammonia molecule and the ammonium ion.

Which type of structure would you expect a hard grey solid which conducts electricity and melts at 3410^oC to have?

ionic (giant lattice)

Which type of structure would you expect a liquid which conducts electricity and solidifies at -39^oC to have?

metallic (giant lattice)

Draw an ionic dot-and-cross for sodium nitride, Na₃N

Draw an ionic dot-and-cross for aluminium fluoride, AlF₃

State two factors that affect the charge density of an ion

charge on the ion radius of the ion

Write a word equation and a balanced chemical equation for the action of heated magnesium on steam

magnesium + steam --\> magnesium hydroxide + hydrogen Mg_(s) + 2H₂O_(g) --\> Mg(OH)_2(s) + H₂_(g)

Write a word equation and a balanced chemical equation for the neutralisation of hydrochloric acid with calcium oxide

calcium oxide + hydrochloric acid --\> calcium chloride + water CaO_(s) + 2HCl_(aq) --\> CaCl_2(aq) + H₂O_(l)

Write a word equation and a balanced chemical equation for the thermal decomposition of beryllium carbonate

beryllium carbonate --\> beryllium oxide + carbon dioxide BeCO_3(s) --\> BeO_(s) + CO_2(g)

Write a word equation and a balanced chemical equation for the action of sulfuric acid on barium hydroxide

barium hydroxide + sulfuric acid --\> barium sulfate + water Ba(OH)₂_{(aq or s)} + H₂SO₄_(aq) --\> BaSO_4(s) + 2H₂O_(l)

Write an equation for the first ionisation enthalpy of calcium

Ca_(g) --\> Ca⁺_(g) + e^-

Write an equation for the second ionisation enthalpy of calcium

Ca⁺_(g) --\> Ca²⁺_(g) + e^-

Write an equation for the third ionisation enthalpy of calcium

Ca²⁺_(g) --\> Ca³⁺_(g) + e^-

The first, second, and third ionisation enthalpies of calcium are +596kJ mol^-1, +1160kJ mol^-1, and +4930kJ mol^-1 respectively Explain why the second ionisation enthalpy of calcium is larger than its first ionisation enthalpy

Once an electron has been removed the remaining electrons are held more tightly. Hence it is more difficult to remove a second electron

The first, second, and third ionisation enthalpies of calcium are +596kJ mo^l-1, +1160kJ mol^-1, and +4930kJ mol^-1 respectively Explain why there is a very sharp rise between the second and third ionisation enthalpies of calcium

Second ionisation enthalpy involves removal of an electron from shell 4 but third involves removal of an electron from shell 3 which is closer to the nucleus

Complete the table that shows the concentrations of ions in water from a sample of Dead Sea water

Calculate the mass of solute needed to make up 1 dm³ of a 2 mol dm^-3 solution of NaCl

117g

Calculate the mass of solute needed to make up 250 cm³ of a 0.1 mol dm^-3 solution of KMnO₄

3.95g

Calculate the mass of solute needed to make up 50 cm³ of a 0.5 mol dm^-3 solution of KOH

1.4g

Calculate the mass of solute needed to make up 15 dm³ of a 2 mol dm^-3 solution of Pb(NO₃)₂

9930g

Calculate the mass of solute needed to make up 10 cm³ of a 0.01 mol dm^-3 solution of LiOH

0.0024g

In a titration, 25.00 cm³ of a sodium hydroxide solution were pipetted into a conical flask. A 0.10 mol dm^-3 solution of sulfuric acid was run from a burette into the flask. An indicator in the flask changed colour at an average of 22.00 cm³ of the acid added H₂SO₄_(aq) + 2NaOH_(aq) --\> Na₂SO_4(aq) + 2H₂O_(l) What is the concentration of the sodium hydroxide solution in mol dm^-3?

4.4 x 10^-3 moles of NaOH_(aq) in 25cm³ gives concentration 0.176 mol dm^-3

In a titration, 25.00 cm³ of a sodium hydroxide solution were pipetted into a conical flask. A 0.10 mol dm^-3 solution of sulfuric acid was run from a burette into the flask. An indicator in the flask changed colour at an average of 22.00 cm³ of the acid added H₂SO_4(aq) + 2NaOH_(aq) --\> Na₂SO_4(aq) + 2H₂O_(l) The student washes the conical flask with water between titrations and does not dry it. Explain the effect, if any, on the titre of the next titration.

No effect on next titre because pippette delivers same amount of NaOH_(aq) as before

A standard solution of sodium hydroxide cannot be made by direct weighing of the solid Explain the meaning of the term standard solution.

A solution of accurately known concentration

A standard solution of sodium hydroxide cannot be made by direct weighing of the solid Suggest why sodium hydroxide cannot be made by direct weighing of the solid

Solid NaOH has the property of absorbing water (and carbon dioxide) from the air so it is not possible to accurately weigh NaOH