Atomic structure Questions and Answers

For a set of quantum numbers where n=2 and 1=1, what are the allowed values of mi? Select the correct answer below: 2,-1,0, +1, +2 -1,0, +1 -3, -2,-1, 0, +1, +2, +3 0

Which is NOT a postulate of Bohr's model of the atom? Select the correct answer below: Electrons are in stationary states. Electrons in a stationary state have a fixed energy. Electrons can change energy by changing their stationary state. Electrons spiral into the nucleus.

Write the full electron configurations of cobalt metal, Co, and one of its ions, Co³+. electron configuration of Co: electron configuration of Co³+: Are Co and Co³+ diamagnetic or paramagnetic? Co is paramagnetic and Co³+ is diamagnetic. Both Co and Co³+ are diamagnetic. Both Co and Co³+ are paramagnetic. Co is diamagnetic and Co³+ is paramagnetic.

What is an atomic orbital? Select the correct answer below: The exact path an electron travels around the nucleus. A region in space where the electron is likely to be found. The location in the nucleus where the proton is found. An area in the atom where the electron overlaps with the proton.

What volume of carbon dioxide is produced when 47.1 g of calcium carbonate reacts completely according to the following reaction at 25 °C and 1 atm? calcium carbonate (s)-calcium oxide (s) + carbon dioxide(g)

In the Bohr model of the hydrogen atom, electrons are confined to orbits with fixed radii, and those radii can be calculated. (a) If an electron makes a transition from the n₁ =4 level to a lower-energy level, nf = 3, 2, or 1, which transition would produce a photon with the shortest wavelength? (b) What are the energy and wavelength of such a photon, and in which region of the electromagnetic spectrum does it lie?

On a climb up Mount Whitney, the atmospheric pressure drops to 529 mmHg. What is the pressure in terms of the following units?

Considering its placement of the Periodic Table and the diagonal filling diagram, give the predicted electron configuration for an element with 44 electrons. Predicted means the electron configuration you would get if you followed your diagonal filling or used the block filling from the Periodic Table as instructed in this course. [kr]5s²4d6 [Xe]5s¹4d7 [Kr]5s¹5d7 [kr]5s²5d6 [Kr]5s24f145d6 [kr]5s23f144d6

Write the electron configuration for Ra and identify how many electrons it has that are in the principal quantum number 6. 32 16 36 02 10 18 08

Write the electron configuration for germanium (Ge) and answer the following questions: a) How many electrons does germanium (Ge) have that are past its nearest noble gas? b) How many electrons have n=3 in Ge? c) How many electrons have spherically shaped orbitals in Ge?

Only using periodic trends, which of the following atoms is predicted to be the smallest? O Se O As OI OK Rb

Given the following nuclear reaction: 257 Fm → 100 Column A 1. 2. 3. 4. — ▬▬▬▬▬▬▬▬ ▬▬▬▬▬▬▬▬▬▬▬ — + 4X What is the atomic mass of the new atom? What is the atomic number of the new atom? What is the symbol of the new atom? What type of decay is demonstrated here? Column B a. Beta Decay b. 256 c. Md d. 99 e. Es f. Gamma Decay g. Alpha Decay h. 257 1. 258 j. 101

Write the electron configuration for selenium (as you did in the question above) and answer the following questions. • How many electrons does Se have in total? . How many valence electrons does Se have? • How many core electrons does Se have? • How many electrons are in n=1? • How many electrons does it have in n=2? • How many electrons does it have in n=3? . How many electrons does it have in n=4? • What is the charge of the ion formed by Se? ● How many electrons are in the electron configuration of this ion? electrons electrons electrons electrons • What noble gas has the same electron configuration as this ion?

Give the electron configuration for fluorine (F). Put the number/letter orbital designation in the first box and the electrons in the superscript box. So, helium would have 1s in the first box and 2 in its superscript box to represent 1s². • How many total electrons does fluorine have? superscripts to check) • How many total electrons does fluoride (F) ion have? . Give the complete electron configuration of fluoride ion. (add the The fluoride ion has the same electron configuration as an atom of

Classify the electron configurations of neutral atoms based on whether they represent an excited-state configuration or a ground-state configuration. [Ar]4s¹3d [Ar] 4s¹3dº: Excited state [Ne]3s23p² [Kr] 5s¹4d10. Answer Bank [Kr]5s¹4d10 1s 2s 2p 3s 3p 3d10424p4 Ground state Which neutral atom has the excited- or ground-state electron configuration, [Ar] 4s¹3d ? Enter the name of the element. [He]2s¹2p4 Which neutral atom has the excited- or ground-state electron configuration, [Kr] 5s¹4d10 ? Enter the name of the element.

If the half-life of substance Z is 2.5 years, how long would it take for 48 grams of substance Z to decay such that only 3 grams remain? years Do not include units in your answer.

Use the following equation to solve this problem: Zett = Z − S where Zeff is the effective nuclear charge, Z is the actual nuclear charge, and S is the screening constant. Among elements 1 to 18, which element or elements have the smallest effective nuclear charge? Check all that apply. H Li Na He Be Mg B Al C Si N S F Cl Ne Ar

Total number of electrons is a subshell is designated by (21+1), where I is azimuthal quantum number.REASON (R)- I can have value 0, 1,2.....n-1,where n is principal quantum number. a b c d

What value do you estimate for Zeff experienced by the outermost electron in both Na and K by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? Express your answers using one significant figure separated by a comma. Zeff Na, ZeffK = What values do you estimate for Zeff using Slater's rules? Express your answers using two significant figures separated by a comma.

Complete the following nuclear equation for Xe-118 which undergoes positron emission. (Determine the new nucleus X?) (1 point) 118 Xe 54 Radioactive Nucleus X + New Nucleus? 0 +1e Positron Radiation

Use the following diagram to answer questions a-d: Infrared (~ 104 m) red (~ 10-6 m) blue (~ 10-7 m) ultraviolet (~ 10-8 m) E n=3 n=2 n=1 C d 9 h a. Compare the energies of the three transitions a, c, & d. Order them from largest to smallest energy. b. Without calculating anything, how would the frequency of transition a compare to transition d? Explain your reasoning. c. Describe what happens to the electron (in terms of energy) before, during, and after transition b happens. Explain your reasoning.

The aqua color line of the Balmer series occurs at 486.1 nm, a. Determine the frequency associated with the photon associated with this wavelength.

Light of wavelength 400 nm strikes a clean surface of metallic Cs in vacuum and ejects an electron having a kinetic energy of 1.54 x 10-19 J. What is the de Broglie wavelength of this electron? O 1.25 nm O 1290 nm O 579 nm 4.72 x 1015 nm

Which of the following is a prediction of the quantum mechanical model of the hydrogen atom but NOT of the Bohr atom? O The number of discrete states that the electron can occupy for each energy level (value of n) increases as n becomes larger. On average, the electron in the hydrogen atom is further from the nucleus in higher energy (higher n) states. O The electron in the hydrogen atom does not fall into the nucleus. O The hydrogen atom absorption spectrum is composed of discrete lines.

Each electron configuration below (i - iii) violates one of the experimentally determined rules for atomic orbital filling. (1) 2p 1 2s 1 Is ↑↓ Filling in the blanks, (i) violates [Select] (ii) 2p ↑↓↑↑ 2s ↑↓↓ Is 1 [Select] , and (iii) violates [Select] (iii) 2p ↑ ↑ 2.s 1 Is ↑↓ (ii) violates. >

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. n=3,1=2, ml=-3 On=2,1=2,m1=0 On=2,1=2, ml=-1 On=4,1=3, m1=-2

Calculate the mass of precipitate formed (in grams) when aqueous solutions of the following reactants are mixed. Assume the reaction goes to completion. 9.50 g of sodium sulfate and 35.7 mL of 0.525 M barium chloride Do NOT include units in your answer. If you round during your calculations, make sure to keep at least four (4) decimal places. Report your final answer to two (2) decimal places. Answer:

8. What is the maximum number of electrons that can be contained within the region (energy level, sublevel, orbital) specified by the following quantum numbers? (3 Marks) [C] a) n=2 Your answer b) n=4, l=1 Your answer c) n=2, l=1, ml=-1 1 point 1 point 1 point

21. The magnitude of the London dispersion forces is proportional to which of the following? O the number of double ionic bonds O ionic bonding O molecular mass of participating molecules O number of single covalent bonds

A ground state hydrogen atom absorbs a photon of light having a wavelength of 93.73 nm. It then gives off a photon having a wavelength of 2624 nm. What is the final state of the hydrogen atom? Values for physical constants can be found in the Chempendix.

Consider a 2170 lb automobile clocked by law-enforcement radar at a speed of 85.5 mph (miles per hour). If the position of the car is known to within 5.0 ft at the time of the measurement, what is the uncertainty in the velocity of the car?

A line in the Balmer series of hydrogen has a wavelength of 656 nm. From what state did the electron originate? n₁ = In which region of the electromagnetic spectrum is this line observed? ultraviolet O visible Omicrowaves O infrared gamma rays radio OX-rays

1. Explain, with examples, how subatomic particles interact to cause ONE of the following periodic patterns. a. Atomic Radius b. lonization Energy c. Electronegativity

Which statement is correct about the reaction shown? (1 Point) 2 SO₂(g) + O₂(g) -> 2 SO3 (8) AH = -196kJ O196 kJ of energy are released for every mole of SO2(g) reacted. O 196 kJ of energy are absorbed for every mole of SO2(g) reacted. O 98 kJ of energy are released for every mole of SO2(g) reacted. 98 kJ of energy are absorbed for every mole of SO2(g) reacted.

Using Heisenberg's uncertainty principle, calculate the uncertainty in the position of a 1.50 mg mosquito moving at a speed of 1.30 m/s if the speed is known to within 10.01m/s. Express your answer using one significant figure. Ar > AΣO Submit Previous Answers Request Answer X Incorrect; Try Again; 19 attempts remaining Part B ? m Using Heisenberg's uncertainty principle, calculate the uncertainty in the position of a proton moving at a speed of (4.80 ±0.01) x 10¹m/s. (Take the mass of a proton m = 1.673 x 10-27 kg.)

An electron is accelerated through an electric potential to a kinetic energy of 2.13 x 10-15 J. Part A What is its characteristic wavelength? [Hint: Recall that the kinetic energy of a moving object is E = mv², where m is the mass of the object and v is the speed of the object.]

Learning Goal: To learn the restrictions on each quantum number. Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. The principal quantum number n corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an electron in the 2p subshell has a principal quantum number of n = 2 because 2p is in the second shell. The azimuthal or angular momentum quantum number & corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, das 2, and fas 3. For example, an electron in the 2p subshell has = 1. As a rule, l can have integer values ranging from 0 to n - 1. The magnetic quantum number me corresponds to the orbital in which the electron is located. Instead of 2pz, 2py, and 2pz, the three 2p orbitals can be labeled -1, 0, and 1, but not necessarily respectively. As a rule, me can have integer values ranging from -l to +l. The spin quantum number m, corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas -1/2 means a "down" spin. ▼ What is the only possible value of my for an electron in an s orbital? Express your answer numerically. ► View Available Hint(s) 0 Previous Answers Part B ✓ Correct Since the allowed values for my range from - to +l, once you know the value for you know the values for l me. Review I Constants I Periodic Table What are the possible values of me for an electron in a d orbital? Express your answer numerically with sequential values separated by commas. ► View Available Hint(s)

List the following types of electromagnetic radiation in order of decreasing wavelength. Rank labels from longest wavelength to shortest. the gamma rays produced. by a radioactive nuclide used in medical imaging the yellow light from sodium vapor streetlights radiation from an FM radio station at 93.1 MHz on the dial the red light of a light-emitting diode, such as in a calculator display Reset a radio signal from an AM radio station at 680 kHz on the dial Help

What is the maximum number of electrons in an atom that can have the following quantum numbers? ♥ n = 3, me =-2 Express your answer as an integer. Number of electrons = VAE Submit Previous Answers Request Answer X Incorrect; Try Again; 19 attempts remaining Part B n = 4, l=3 Express your answer as an integer. ? Review | Constants

Dimensional Analysis 2: Molar Concepts: Question 3 One mole of NaCl and one mole of Cl₂ have a mass of 1 gram each contain the same number of molecules have the same mass contain one molecule each

The compounds SO3 and PF3 have similar chemical formulas, but they have different molecular shapes. Why do these compounds have different molecular shapes? Compare the structures of the compounds, discuss their similarities and differences, and explain the reason for the differences.

Which two neutral atoms would have the same number of valence electrons, according to the highest ns*npy in their electron configurations? chlorine oxygen phosphorous sodium sulfur calcium

Match each subshell (s, p, d, and f) with the maximum number of electrons it can hold. p [Choose] d [Choose ] f 4 electrons s 2 electrons 12 electrons 14 electrons 10 electrons 16 electrons 6 electrons 8 electrons

Consider this ionic isotope. The identity of the element is missing. 39 ? 2+ 20 Which three statements are true? It's calcium It's a cation It's an anion It has more than 17 neutrons It's yttrium It has gained two electrons The nuclear charge is 39 The mass number is 20

How many atoms are in 4.28 g of yttrium? Select the correct answer below: 1.25 x 1025 atoms 2.58 x 1024 atoms 5.35 x 1025 atoms 2.90 x 1022 atoms

Indicate which is larger in each of the following two sets. (I) Cr3+ or Cr (II) Se2- or Se A) Cr3+ is larger than Cr and Se2- is larger than Se. B) Cr3+ is larger than Cr and Se is larger than Se2-. C) Cr is larger than Cr3+ and Se2- is larger than Se. D) Cr is larger than Cr3+ and Se is larger than Se2-.

How many moles of copper (II) sulfate (CuSO4) are in a 0.125 g sample of CuSO4? • Your answer should have three significant figures.

Four iron (II) ions, Fe2+, are the key components of hemoglobin, the protein that transports oxygen in the blood. Assuming that these ions are 53Fe2+, how many protons and neutrons are present in the nucleus and how many electrons are present in each ion

What led Rutherford to believe that atoms contained a positive nucleus? Most alpha particles went straight through the gold foil Some alpha particles were deflected by the gold foil The line spectra of excited atoms Atoms are electrically neutral

Compute the following and give your answer in scientific notation: (Round to the nearest hundredth.) (6.77 x 10³) + (5.85 x 10³) = × 10^