Below are the first 6 ionization energies for an element in kJ/mol.IE1IE2IE3IE4IEAIE5IE,57818171157714842183792745Identify the element.A. o aluminumB. o sodiumC. o phosphorusD. o magnesiumЕ.silicon

Ionization energy is the minimum energy required to remove an electron from the outermost shell of…

IE6 Below are the first 6 ionization energies for an element in kJ/mol. IE, IE, IE3 IE4 IE5 IE, 578 1817 2745 11577 14842 18379 Identify the element. A. o aluminum B. o sodium C. o phosphorus D. o magnesium E. o silicon

IE6 Below are the first 6 ionization energies for an element in kJ/mol. IE, IE, IE3 IE4 IE5 IE, 578 1817 2745 11577 14842 18379 Identify the element. A. o aluminum B. o sodium C. o phosphorus D. o magnesium E. o silicon

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 145AE: The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 =...

See similar textbooks

Related questions

Q: n=00 n=4 In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. n=3…

A: In this transition electron moves from n=4 level to n= 1 level

Q: 81.) Arange the following sts of elements in order of increusing atomic size. a Sn, Xe, Rb,Sr b. Rn,…

A: We need to arrange all these elements in increasing atomic size . Atomic size varies differently in…

Q: Choose the element with the larger atoms from each pair.(a) Al or In (b) Si or N(c) P or Pb (d) C or…

A: Increasing order of size: (a) Al < In (b) N < Si (c) P < Pb (d) F < C…

Q: How many subshells are in the n = 3 shell? subshells How many orbitals are in the n = 3 shell?…

Q: What is the maximum number of electrons in each of the following sublevels? (a) 2s (b) 4p (c) 3d.…

A: To find: The maximum number of electrons in each of the given sub level.

Q: On a remote island in the Arctic Ocean, a scientist claims to have found a new element (Excitinium)…

A: Given: On a remote island in the Arctic Ocean, a scientist claims to have found a new element…

Q: How many electrons in an atom can have each of the following quantum number or sublevel…

A: How many electrons in an atom can have each of the following quantum number or sublevel designations…

Q: For the quantum number, indicate if it is possible or not. If not possible, give an explanation. n…

A: Given: n = 4 l = 3 ml = -2 ms = +1/2

Q: This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI…

Q: 212. Explain the following diagram (a) and (b) and compare two models and associated heories…

A: These are the models of JJ Thomson and Ernest Rutherford.

Q: How many sublevels are in the n = 3 level? sublevels: How many orbitals are in the n = 3 level?…

A: Given, n=3 level andwe are asked to the number of sublevels, orbitals and maximum number of…

Q: (D) 8.59 mL 2. Consider the Bohr Model of Phosphorus below. Which statement is FALSE? (A) The…

A: Postulates of Bohr’s Model of an Atom: In an atom, negatively charged electrons revolve around the…

Q: Identify the subshell in which electrons with the following quantum numbers are found: n=4, 1=2

A: n is called the principal quantum number and it gives information regarding the shell in which…

Q: The number of electrons in the highest energy level of 20Ca is a. 2 b. 4 c. 5 d. 6 e.…

A: The atomic number of calcium is 20 and it is a group 2 element. The electronic configuration of…

Q: Find the atom that is most likely (energetically) to lose an electron: Na S Li Mg

A: The ions formed after loosing an electron: Na→Na+ + e- S→ S+ + e- Li→Li+ + e- Mg→ Mg+ + e-

Q: The spheres below represent atoms of Sb, As, P, and N (not necessarily in that order). r-75 pm (a)…

A: Along the period force of attraction between proton and electron is increases. Along the group…

Q: = 4 Which of the electron transitions would release the most energy? A) I B) II C) III

A: When electron makes a transition between energy levels then it emit and absorb energy. When…

Q: 2. The Main Energy Level is composed of P, d, and f: A.Pauli's Exclusion Principle B. Hund's Rule…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 1. Write down the following rules, in your own words: a. Aufbau principle b. Pauli Exclusion…

A: Since your question has multiple parts, we will answer the first question for you. If you want…

Q: For the quantum number, indicate if it is possible or not. If not possible, give an explanation. n…

A: QUANTUM NUMBERS: The set of numerical that are used to define the energy of the electron and the…

Q: 5. Of the elements B, Al, and S, which has the largest atomic radius and why? A. boron because it…

A: Atomic radius increases down the group and decreases across the period because along the period…

Q: How many energy sublevels are found in the 15t energy level? O a. 1 O b.2 Oc3 O d.4

A: As we know that quantum energy levels are that levels in which electrons are present , inside every…

Q: Rank the following atoms in order of decreasing size (i.e., largest to smallest): Rb, F, Mg, В, N.…

A: Option A) Rb > Mg > B > N > F is correct.

Q: Select the correct sequence of the elements Al, K, Mg and N in order of decreasing atomic size.

A: Atomic size increases down the group in periodic table. Atomic size decreases from left to right in…

Q: Which of the following statements concerning the Pauli exclusion principle is/are CORRECT? 1.…

A: According to Pauli Exclusion Principle,

Q: Arrange the following groups of atoms in order of increasing size. a.) Cs, Mg, K b.) Sb, Ba, S c.)…

A: (a) Atomic size decreases along a period and increases down a group. Alkali metals have the largest…

Q: What type of sublevels (s,p,d,f) are present in n=2? O only the s-sublevel O s,p,d, and f O s and p…

A: There are 4 quantum numbers that define the complete configuration of the system. 1). Principal…

Q: In an atom, how many electrons can be assigned the principal quantum number n = 4 and the spin…

A: All things are provided in handwritten solution

Q: 23. Recall the simulation on Bohr and Quantum Model of the atom. What elements were found to be in…

Q: On the blank Bohr Models, create a model for Sodium-23 and Sodium-25. When finished, describe the…

Q: What is the maximum number of electrons that a d subshell can contain? O 14 10 2 6.

Q: Fill in the information missing Some electron shells shell subshells 2 2.s, 2p 4 1

A: Given that : We have to fill the missing information in the following table:

Q: According to the Bohr model, when a hydrogen electron makes a transition from n=4 to n=2, which of…

A: Given : Bohr model of hydrogen atom. To find : True statements. Solution : As we know, when a…

Q: The maximum number of electrons that can be accommodated in a sublevel for which I = 3 is: Select…

A: Quantum numbers are the hypothetical numbers used to designate the location of of electron in an…

Q: n=4 V In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. n=3 One…

A: According to Bohr`s atomic theory, electrons in an atom move from a lower energy level to a higher…

Q: 2. Which is TRUE about the 3p electrons in sulfur? (A) They travel in a figure 8 orbit (B) They are…

A: The increase in shell number energy also increases

Q: What is the total number of electrons in the second principal energy level of calcium in the ground…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: How many occupied sublevels are in an atom of carbon in the ground state? a) 5 b) 6 20. c) 3 d) 4…

Q: The spheres below represent atoms of Li, Be, B, and F (not necessarily in that order) r- 112 pm r-83…

Q: 3) Consider element "X": 13 X a) How many protons does X3* have? b) How many neutrons does X³* have?…

A: Element 3 is most likely representing the values for I.E. (ionization energy) for X and from the…

Q: gives the correct numbers of subatomic particles in an atom of an element with atomic number (Z) 48…

A: 1) Atomic mass = number of protons = 48 Mass number = 120 Number of Neutrons = 120 -48 = 72…

Q: Arrange atoms C, K, Ge, Cs in order of: decreasing atomic size:

A: Distance from the centre of nucleus of an atom to the outermost shell is termed as atomic size.

Q: 4. The diagram shows the lowest two energy levels of an atom. B 2.4 x 10-19 J A - Use the constants…

A: Energy is inversely proportional to wavelength.

Q: How are the electron configurations of F, 02, and Na* similar?

A: 1. Fluorine on gain of 1 electron forms F- Electron Configuration of F- F- = [He] 2s2 2p5 2. Oxygen…

Question

Below are the first 6 ionization energies for an element in kJ/mol.
IE1
IE2
IE3
IE4
IEA
IE5
IE,
578
1817
11577
14842
18379
2745
Identify the element.
A. o aluminum
B. o sodium
C. o phosphorus
D. o magnesium
Е.
silicon

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

6.101 Laser welding is a technique in which a tightly focused laser beam is used to deposit enough energy to weld metal parts together. Because the entire process can be automated, it is commonly used in many large-scale industries, including the manufacture of automobiles. In order to achieve the desired weld quality, the steel parts being joined must absorb energy at a rate of about 104 W/mm2. (Recall that 1 W = 1 J/s.) A particular laser welding system employs a Nd:YAG laser operating at a wavelength of 1.06m ; at this wavelength steel will absorb about 80% of the incident photons. If the laser beam is focused to illuminate a circular spot with a diameter of 0.02 inch, what is the minimum power (in watts) that the laser must emit to reach the 104 W/mm2 threshold? How many photons per second does this correspond to? (For simplicity, assume that the energy from the laser does not penetrate into the metal to any significant depth.)
Explain the main features of Bohrs theory. Do these features solve the difficulty alluded to in Question 7.8?
The “Chemistry in Focus" segment The Chemistry of Bohrium discusses element 107. bohrium (Bh). What is the expected electron configuration of Bh?
6.83 The graph below shows the first three ionization energies for sodium, magnesium, and aluminum. Without consulting a list of values, determine which line in the graph corresponds to each element. Number of electrons removed
The following are orbital diagrams for presumed ground-state atoms. Several, though, violate Paulis principle or Hunds rule Which of the these follow both Paulis principle and Hunds rule, and which violate one or the other (state whether Paulis principle or Hunds rule is violated)? a b c d e
Give electron configurations according to the Bohr model for each of the following elements. Try to not use Figure 3.11, but instead determine the configuration based on your knowledge of the number of electrons in each atom and the maximum number of electrons in each Bohr orbit. Indicate which of these elements you expect to be the most reactive and the least reactive. a. B b. Si c. Ca d. F e. Ar
An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.
Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what evidence was there that it "works"? Why do we no longer "believe" in it?
Give electron configurations according to the Bohr model for each of the following elements. Indicate which of these elements you expect to be the most reactive and the least reactive. a. He b. Al c. Be d. Ne e. O
The ionization of the hydrogen atom can be calculated from Bohr's equation for the electron energy. E = (NARhc)(Z2/n2) where NARhc =1312 kJ/mol and Z is the atomic number. Let us use this approach to calculate a possible ionization energy for helium. First, assume the electrons of the He experience the full 2+ nuclear charge. This gives us the upper limit for the ionization energy. Next, assume one electron of He completely screens the nuclear charge from the other electrons, so Z = 1. This gives us a lower limit to the ionization energy. Compare these calculated values for the upper and lower limits to the experimental value of 2372.3 kJ/mol. What does this tell us about the ability of one electron to screen the nuclear charge?
The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 = 14,807 kJ/mol I4 = 17,948 kJ/mol To which family in the periodic table does the unknown element most likely belong?
Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found to be incorrect. c. The hydrogen atom has quantized energy levels. d. An orbital is the same as a Bohr orbit. e. The third energy level has three sublevels, the s, p, and d sublevels.