Atomic structure Questions and Answers

22 Given the reaction 2 Mg s O g 2 MgO s What is the minimum number of moles of Mg required to produce 1 mole of MgO 23 A Go over combustion reaction of methane CH4 B If 16 0 g of methane gas is burned completely what would be the expected mass of carbon dioxide and water Mass of oxygen consumed

A certain form of lead has a cubic closest packed structure with an edge length of 492 pm Calculate the value of the atomic radius and the density of lead Atomic radius Density m g cm

a Calculate the heat required to melt 5 50 g of benzene at its normal melting point Heat of fusion benzene 9 92 kJ mol Heat b Calculate the heat required to vaporize 5 50 g of benzene at its normal boiling point Heat of vaporization benzene 30 7 kJ mol Heat k c Why is the heat of vaporization more than three times the heat of fusion O More energy is required to overcome the forces holding the molecules together in the liquid state to g than to just allow the molecules to begin mov O Forces holding molecules in the liquid state are much stronger than in the solid state O In the liquid state intermolecular forces must be broken while in the solid state intramolecular forces must be broken

3 Using the Bohr Diagram in your reference packet answer the following questions a What is the wavelength of light emitted when an electron moves from n 3 to n 1 b What is the type of light emitted

The energies E for the first few states of an unknown element are given in the table in arbitrary units 1 2 3 4 11 5 2 1 11 E Photon A A gaseous sample of this element is bombarded by photons of various energies in these same units Match each photon to the result of its absorption or lack thereof by an n 1 electron B C D Energy 11 9 8 6 Result 0000 0 Answer Bank n 1 to n 3 not absorbed electron ejected n 1 to n 4 n 1 to n 2

A few different types of electromagnetic radiation are listed in the table below Complete the table by ordering these types of radiation by increasing frequency wavelength and energy per photon For example select I in the second column for the type of radiation with the lowest frequency 2 for the type of radiation with the next higher frequency and so forth type of radiation blue light X rays red light Infrared radiation order of frequency Choose one Choose one Choose one Choose one order of wavelength Choose one Choose one Choose one Choose one order of energy Choose one Choose one Choose one Choose one

2 11 Why is a molecule of CO nonpolar even though the bonds between the carbon atom and the oll oxygen atoms are polar 1 The shape of the CO2 molecule is symmetrical 3 The CO2 molecule has a deficiency of electrons The shape of the CO2 molecule is asymmetrical 4 The CO2 molecule has an excess of electrons

21 Rank the following bonds from the strongest to the weakest Make 1 the strongest and 6 the weakest Van der Waal Forces Ionic Bonds Single Covalent Bonds Double Covalent Bonds Hydrogen Bonds 3 Triple Covalent Bonds

31 Which statement explains why H O has a higher boiling point than N 1 H O has greater intramolecular forces than N 3 H O has stronger intermolecular forces than N binor inal diod E 2 H O has less intramolecular forces than N vino 4 H O has weaker intermolecular forces than N2

O isotopes O ions of the same element must have different numbers of neutrons electrons O electron orbitals shells valences

What is the mass number of an isotope with an atomic number of 55 and that has 67 neutrons

The mass number of an element is equal to 1 The number of neutrons in an atom 2 The number of electrons in an atom 3 The number of protons in an atom 4 The number of isotopes in an atom 5 The number of protons and neutrons in an atom

Which of the following always increases as you move from left to right across a row in the periodic table Atomic number Number of neutrons O Number of isotopes Atomic mass

How many valence electrons are in an atom of chlorine

1 Jeannie is an experienced business traveler often traveling back and forth from San Francisco to the East Coast several times per month To catch her flights from San Francisco she leaves her office one hour before her flight leaves Her travel time from her office to the departing gate at the San Francisco airport including the time to park and go through security screening is normally distributed with a mean of 46 minutes and a standard deviation of 5 minutes What is the probability that Jeannie will miss her flight because her total time for catching her plane exceeds one hour 0 0017 0 0026 0 0059 000137

Q16 Which one of the following is an incorrect orbital notation A 4f B 2d A NaCl and Ca NO3 2 C 3s D 2p D None of them Q17 Which reactants will produce a precipitate when mixed in aqueous solution B BaCl and Na3PO4 C NaOH and HCI

Q4 What is the frequency s of radiation that has a wavelength of 459 nm A 6 54 x 10 B 6 54 x 10 C 1 53 10 Q5 Which one of the following is not a redox reaction A 2H 02H O Oza C BaCl K CrOBaCrO KCl B 2 16 x 10 m D 18 10 V B Na 3H 2NH D 2Al Fe O Al O 2Fe Q6 What are the reacting ions when Pb NO and NaCl react in aqueous solution A Pb Cit B Na NO C Pb NO D Na Cl Q7 The correct order of increasing in the first ionization energy A B Be N O D B O Be N C B Be O N B Be B N O Q8 What is the A of light that is emitted when an excited electron in the hydrogen atom falls from n 7 to n 47 A 4 45 x 10 m C 9 18 x 100 m D 2 16 x 10 m

What is the maximum number of electrons a g orbital 2 There is no such thing as a g orbital 18 9 can hold

How many orbitals are there in the 2nd energy level 4 8 6 2

What is the level of heavy metal in ppm in a 3 89 kg sample that has 0 9 mg of the heavy metal present in the sample 1 kg 1 000 000 mg

What is the mass number for the following ion 195 Au 79 76 197 70 79 195

2 point Which of the following is the correct shorthand electronic configuration for Molybdenum Mb O O O O Kr 5s 4d5 Kr 4d6 Kr 4d4 kr 5s 4d4

Which of the following represents the correct ground state electron configuration for Se O a 1s21p62s22p63s23p64s23d104p4 b None are correct O c 1s22s22p63923p64s23d104p4 O d 1s21p62s22p63923p64s 4p4 e All are correct

Of the following atomic orbitals which has the highest energy O a 3d Ob 3s O c 3p O d 4s e 2s

What is the maximum number of electrons the 6th energy level can hold The 6th energy level does not exist O 36 O 72 6 Previous

Which correctly represents atom X which has 50 protons 63 neutrons and 50 electrons O a None of these W Ob x presubscript 50 presuperscript 113 superscript blank OCX presubscript 50 presuperscript 113 superscript 13 plus end superscript OdX presubscript 63 presuperscript 50 superscript 13 plus end superscript X presubscript 50 presuperscript 63

What is the correct valence electron configuration for P O a 1s22s22p63s23p3 Ob 1s22s22p63s23p5 OC 192288385 Od None are correct O e 3823p3

A neutral atom has the following electron configuration 1s 2s 2p 3s 3p 4s 3d What is the chemical symbol for the atom How many electrons does the atom have How many 3d electrons are in the atom 0 7 X

Use the information below to answer this question Ne These isotopes of Neon have Ne the same number of neutrons and different numbers of protons the same mass number and different atomic masses O the same number of protons and different numbers of neutrons the same number of protons and different numbers of electrons

Refer to the provided Periodic Table to answer this question Which of these electron configurations represents the ground state electron configuration of a d sublevel metal O 1s 2s 2p 3s 3p O 1s 2s 2p 3s O1s 2s 2p 3s 1s 2s 2p 3s s23d204p 05p56s 4f 04p05s 4d4 POS

5 What is the molality of a 351 ppm solution of carbon dioxide in water

22 What is the smallest acceptable value for the missing quantum number n 1 2 m 0 m 1 2

How many electrons can occupy the d sublevel 06 O 10 05 2

Which subatomic particle has no charge and is found in the center of an atom O proton O neutron electron nucleus

What would be the electron configuration for an atom of oxygen in its ground state O 1s 2s 2p6 O 1s 2s 2p4 O 1s 1p 2p 2p O 1s 2s 2p 3s

What is the best explanation for why the electronegativity decreases going down group 1 from hydrogen to francium O The atomic radius decreases O The number of neutrons increases O The number of valence electrons increases O The valence electrons are farther away from the nucleus

Potassium metal K reacts violently when mixed with water and produces potassium hydroxide and hydrogen gas Which metal would most likely react similarly titanium Ti sodium Na aluminum Al magnesium Mg

Reactants Cu 89 Pb s Products Cu ae Mass of solids Pb s 0 892012 g Mass of solids Molarity of metal ag SCH4U Unit 4 Electrochemistry 0 892012 g 0 1 M Molarity of metal ag 3 92983e 7 M Observations Blue liquid Observations Clear Date

2 Locate these metals on the periodic table and give at least two possible reasons for why one metal is a stronger reducing agent than another based on their positions Mg Zn Pb Cu

For each atom in the table below write down the subshell from which an electron would have to be removed to make a 1 cation and the subshell to which an electron would have to be added to make a 1 anion The first row has been completed for you atom H Ga Li He subshell from which electron removed to form 1 cation 1s 0 0 7 subshell to which electron added to form 1 anion Is 0 0 E

Graph the following Data for the elements in Period 3 This will help us understand how atomic radius ionization energy and electronegativity as you go across a group and see what the trends are You will need to make three separate graphs One for atomic radius one for lonization Energy and one for Electronegativity Make the x axis the atomic numbers of the elements and the y axis the data from the chart Make sure you give each chart a title and label the axis Symbol Na Mg AI Si P S CI Ar Atomic Radius Picometers 166 141 121 111 107 105 102 106 First lonization kilojoules mole 496 738 578 787 1012 1000 1251 1521 Electronegativity 4 point scale 09 1 2 1 5 1 8 2 1 2 5 3 0

1 Be sure to answer all parts How many protons neutrons and electrons are contained in the atom with the given atomic nur and mass number Z 13 A 26 Protons Neutrons Electrons

5 Be sure to answer all parts Complete the table of isotopes each of which has found use in medicine a Sodium 24 b select Atomic number Mass number Number of protons 24 Number of neutrons 27 Isotope symbol

the molarity if you have 89 9 grams of potassium bromide and 900mL 7 A teacher tells a student to make 1000mL of a 0 50M solution of calcium chloride What mass will need to be measured out to complete this task

1 2 Which of the following molecule has largest radius a P b S d Se Which of the following atom or ion has smallest radius a N b O d p3 As C energy d P 3 The energy required to remove an electron from a gaseous atom is called a ionization potential electron affinity c electronegativity b d lattice

3 An electron in the hydrogen atom falls from the n 5 state to the n 1 state A 6 pts Calculate the energy released Rydberg constant RH 2 18x10 18J DH RHXC hr 12 np DH 2 18x101x 25 1 AH 2 18 10 3 0 04 1 18 BH 2 093 10 18 50 96 hr 6 13 09 Hame 10 B 6 pts Calculate the wavelength of the light emitted in the transition Speed of ligh 3 0 x108 m s

Rank the following elements in order of increasing ionization energy boron fluorine helium magnesium and potassium He Mg F K B increasing ionization energy 2

29 2 points Which of the following exhibits hydrogen bonding PH3 H CO OH H O2 Previous

10 Rank the following elements in order of decreasing ionization energy potassium aluminum nitrog sodium and boron select select select select select

2 What element has an atomic number of 10 and contains 10 neutrons How many electrons does t atom contain What is its mass number Element select Electrons Mass Number