(a) Which of the following atoms or ions is diamagnetic? Cu2+ Se4+ V2+ Co3+ V4+ (b) Which of the following atoms or ions is paramagnetic? Cl3+ N3+ Mn7+ V5+ Ne

Q: ionization energy

A: Ionization energy is defined as the amount of energy required in order to remove most loosely bound…

Q: Bromine is used in the manufacture of disinfectant products, it has a very strong oxidizing…

A:

Q: A ground-state atom of iron has _____ unpaired electron and is _________a. 0, diamagneticb. 6,…

A: Given,0, diamagnetic6, diamagnetic3, paramagnetic4, paramagnetic5, paramagnetic

Q: The hot glowing gases around the Sun, the corona, can reach millions of degrees Celsius, high enough…

A: There are commonly two main types of magnetism in the compounds. They are paramagnetism and…

Q: The following is the electron configuration of a nonexistent transition metal. electron…

A:

Q: Predict the trend in values of Slater's  constant of the every first element of each group of p…

A:

Q: Which of the following atoms are paramagnetic?  a Zn  b O  c P  d Mg

A: It is explained as given below :

Q: Which atom has the same electron configuration as In? In3+? Ga Zn Pd Ir O Te

A: The element having same number of electrons as In3+ will have same electron configuration as In3+

Q: im not too sure how to fill this out

A: There are four sets of quantum number for a particular electron in an atom :-  principle quantum…

Q: Explain each of the following observations: The halogens decrease in oxidizing power in the order F2…

A: Introduction :  Oxidising power of halogens decreases down the group .

Q: 7 Part B What is the ground-state electron configuration of the sulfide ion S²-? Express your answer…

A:

Q: 2- Which of the following is wrong? O A) The outermost shell electronic configuration of the Kr…

A: The question is based on concept of atomic structure. it involves writing electronic configuration…

Q: In the Fe2+ ion, how many unpaired d electrons are there?

A: The atomic number of Fe is 26  Hence the electron configuration of Fe is [Ar] 3d6 4s2

Q: Two fourth-period atoms, one of a transition metal, M, and the other of a main-group nonmetal, X,…

A: If M is considered as Iron, the general formula given was M2X3, then the compound has to be Fe2X3.…

Q: Calculate the effective nuclear charge on a 5s, a 5p, and a 4d clectron in a tin atom.

A: Effective nuclear charge (Z* ) is calculated using the formula:  Z* = Z - σ Z= Atomic number σ =…

Q: Which of the following species is diamagnetic (not paramagnetic): Li, V, Ni, Zn, Fe-

A: Please find the answer attached.

Q: Q.Arrange the following in their increasing size with the help of slater’s rule and also give…

A:

Q: How many unpaired electrons does [Cr(OH2)6]2+ have when it has a highspin d electron configuration?

A:

Q: How many unpaired electrons would be present on a Be2 2− ion? Would it be paramagnetic or…

A: On Be2 2- ion,there will be two unpaired electrons in the molecular orbitals.As there are two…

Q: Define actinides

A: Actinides have to be defined.

Q: Which transition-metal ion with a 3+ charge has the electron configuration [Kr]4d?

A: Transition metal atom and ions are those elements which lie in between s and p block elements and…

Q: Indicate whether technetium, Z = 43, would be expected to be paramagnetic. Technetium is not…

A:

Q: Which of the following ions has the electron configuration 1s22s22p°? A) Mg* B) N2 C) N3 D) O E) F*

A:

Q: How many unpaired electrons would you expect for chromium in [Cr(H2O)6]3+? Is this a paramagnetic or…

A: To determine the unpaired electrons, first make the orbital diagram of the transition element…

Q: Explain why actinides are colourful (5)

A:

Q: Q1 Write electronic configuration of: Sc*, Cr*3, Mn*7, Fe** Q2which of the above is paramagnetic

A:

Q: Is N22- paramagnetic or diamagnetic?

A:

Q: 9 Which of the following atoms or ions is most paramagnetic? a. b. Zn2+ Gd d. U6+ c.

A: The ions which has most number of unpaired e- in valence shell and outermost shell will have the…

Q: coloured and why? Explain. Example 8. Which of the following ions are expected to be 3+ 2+ Cut,…

A: The element which have unpaired electron is coloured. As unpaired electron can absorb energy and…

Q: What is the ground-state electron configuration for Mn in MnO2? O a. [Ar] 3dº O b. [Ar] 4s2 3d6 O c.…

A: To write the electronic configuration of Mn in MnO2 we have to first determine the oxidation state…

Q: The ground-state electron configuration of, O Fe is [Ar]4s 13d 5. V Cr O K O Mn

A:

Q: Zn and Zn2+ are both diamagnetic.

A: Diamagnetic is nothing but the fully paired electron containing orbitals ie. the oribital must have…

Q: Which of the following fictitious compounds is more likely to be paramagnetic based off of your…

A: A coordination compound will be paramagnetic if the central transition metal or metal ion has at…

Q: Write the general electron configuration of a transition ele-ment (a) in Period 5; (b) in Period 6.

A: General electronic configuration of a transition element (a) in Period 5; (b) in Period 6 has to be…

Q: Which element has the largest bonding atomic radius: Sc,Fe, or Au?

A: In the periodic table the elements are arranged according to their periodicity properties. These…

Q: Which of the following atoms is paramagnetic? A) AI В) Ва C) Kr D) Zn E) Хе

A: Which of the atoms is paramagnetic ?

Q: Which of the following is the electronic configuration of the Chromium(III)? Cr3+ [Ar] 3d3 .a O Cr3+…

A: The Aufbau principle indicates the manner in which electrons are filled in the atomic orbitals of an…

Q: Why is the electronic configuration of the yttrium atom [Kr]4d15s2 and that of the silver atom…

A: Introduction- Electronic configuration means a systematic representation of the arrangement of the…

Q: 15. Explain carefully why cesium tends only to form a +1 ion?

A: Introduction: We have to tell why cesium shows +1.

Q: Which transition metals have a maximum O.N. of +6?

A: Transition metals: These are the elements that have partially filled d subshell. In other words, the…

Q: Which of the following species will be diamagnetic? A) Co2* B) Cr* C) Zrt D) V³+ E) Ni²*

A:

Q: För each of the following ions, draw diagrams (on a piece of paper), like the one to the right…

A:

Q: The number of unpaired electron(s) in F₂ is/are A 4 B 0 C 1 D) 2 E 3

A:

Q: Which metal ion is expected to have the electron configuration, 1s? 2s? 2p6 3s2 3p6 3d10 4s² 4p6 4d4…

A: To identify the metal ion that is expected to have below electronic configuration…

Q: which of the following ion is paramagnetic and coloured in nature: a  Cu^2+ b  Cu^+  c  Zn^2+ d…

A: The paramagnetic compounds or atoms or ions have unpaired electrons and are attracted towards the…

Q: Among the period 4 transition metals (Sc–Zn), which elements do not form ions where there are…

A: The transition element present in the fourth period are Scandium, titanium, vanadium, chromium,…

Q: Which transition-metal ion with a 3+ charge has the electron configuration [Kr]4d5

A:

Q: Paramagnetism is the tendency of an atom to be attracted to a magnet. The more unpaired electrons…

A: we have to arrange the given species in order of increasing paramagnetism

Formal Charges

Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.

Polarity Of Water

In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent. 

Valence Bond Theory Vbt

Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.