Q: Electron affinity - from left to right within a period from top to and _-- bottom within a group. O…
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Q: Name two elements in the group which has the general electron configuration ns2np3.
A: Given: The general electron configuration of element is ns2np3. Here, n represents the principal…
Q: In the isoelectronic series Ca2 + , Cs+, Y3 + , which ion islargest?
A: Among Ca2+, Cs+, Y3+ the largest ion will be:
Q: Ti and Hf behaveas though they possess the same number of valence electrons.Which of the subshells…
A: Electrons from the most outer shell always behave as valence electrons. But if we have elements with…
Q: Consider the first ionization energy of neon and the electronaffinity of fluorine. (a) Write…
A: Ionization energy is the amount of energy which is needed to remove an electron from the neutral…
Q: Consider an ionic compound, MX,, composed of generic metal M and generic, gaseous halogen X. • The…
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Q: Consider the isoelectronic series Zr4+, Nb5+, Mo6+, Tc7+. Arrange these species as follows. (Use the…
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Q: Platinum hexafluoride, PtF6 has a very high electron affinity (772 kJ/mol) but when lithium metal is…
A: Lithium has a very small size and has the maximum polarizing power due to its small radius.
Q: Bromine is used in the manufacture of disinfectant products, it has a very strong oxidizing…
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Q: An element X has the electron configuration [Kr] 5s-4d5p. The formula for the bromide of X is most…
A: The given electronic configuration is [Kr] 5s24d105p3. The atomic number of an element is equals to…
Q: In group 15 elements, there is considerable increase in covalent radius from N to P but small…
A: N i.e nitrogen is period 2 element, P i.e phosphorous is period 3 element, As i.e Arsenic is period…
Q: Use the electron configurations of the alkaline earth metalsto explain why they tend to form 2+…
A: We have alkaline earth metal, we have to explain why they tend to form the +2 ions.
Q: Arrange these ions from largest to smallest ionic radius Ba2+, Cs+, Te2-, I, Sb3-
A: ions from largest to smallest ionic radius is Sb3- >Te2- > I > Cs+ > Ba2+
Q: Rank the following in order of the indicated property. a. N, As, P, Bi (decreasing…
A: Electron affinity is the extent of energy released when an electron is added to a neutral gaseous…
Q: In group 15 elements, there is considerable increase in covalent radius from N to P but small…
A: ANSWER
Q: In the chemical process called electron transfer, an electron istransferred from one atom or…
A: Electron affinity is the amount of energy released on the addition of an electron to a neutral atom.…
Q: Discuss the importance of electron affinity and ionizationenergy in the formation of ions.
A: Electron affinity: release of certain amount of energy when an electron is added to neutral…
Q: Explain the group IV and V cations. Draw their schematic diagram.
A: Elements in the same group have similar outermost configuration and hence ions they form have…
Q: Use electron configuration and orbital diagram to account for the trend in electron affinity from…
A: Electron affinity is the amount of energy released when electron is added to an isolated gaseous…
Q: Why the ionic radii of Zr and Hf are almost equal?
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Q: Explain why each successive ionization of an electronrequires a greater amount of energy.
A: The ionization energy of an element indicates the minimum quantity of energy which is required to…
Q: 20 The generic lonic compound, MX is composed of metal M and gemerie geous halogen X Caleulate its…
A: Lattice energy is the energy released when one mole of an ionic compound is formed from its…
Q: Relate the change in atomic radius to the changesin atomic structure that occur across the…
A: In the periodic table, elements are arranged according to their electronic configuration. As the…
Q: WHAT IS THE ELEMENT: a) of Group 4A, with the most metallic character b) of Group 5A which forms the…
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Q: What are the identidication tests used for the group III and IV elements? Give comprehensive…
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Q: arrange the following in order of increasing radius and increasing ionization enegy n+,n,n-
A: Atomic radius: The distance of the outermost electron from the nucleus is known as the radius of the…
Q: (b) List some properties of Group 1 elements which indicate they are all metals. (c) What valence do…
A: Here we have to write some properties of group 1 metal, valency of group 1 elements and name and…
Q: Write the electron configuration for Si7+ ion.
A: The arrangement of electrons in orbital shells and sub shells is the electronic configuration of an…
Q: Consider the isoelectronic series Ca2+, Sc3+, Ti4+, V5+. Arrange these species as follows. (Use the…
A: Answer :- a) Ionic radius :- It is the distance of the outer most shell of an cation or anion from…
Q: Group the electronic configurations of neutral elements in sets according to those you would expect…
A: The element with electronic configuration 1s2 2s2 2p6 3s2 3p3 and the element with electronic…
Q: Choose two atoms. List what their electron affinity values are including units. Which of these two…
A: I am taking two halogens F and Br atom. Electron affinity of fluorine =-328kj/mol Electron…
Q: Consider an ionic compound, MX,, composed of generic metal M and generic, gaseous halogen X. • The…
A:
Q: Consider a hypothetical ionic compound AB (comprised of A* and B" ions). Given the following…
A: The enthalpy change during the formation of one mole of ionic crystal from one mole of gaseous…
Q: If the left most element in a period combined with each of the others in the period, how would the…
A: A chemical compound consists of two or more different elements which are bonded with each other…
Q: What are the connections between reactivity and ionization energy/electron affinity trends? Why do…
A: There are many trends in organic chemistry. These trends are atomic size, reactivity, metallic…
Q: A – most electronegative element in - Period 4. B - smallest atom in Group 5A. C- alkaline earth…
A: A - most electronegative element in Period 4. Answer : bromine Reason : the tendency to attract…
Q: Consider the elements selenium (Se) and bromine (Br). Whichhas the higher first ionization energy?…
A: From the given two elements which has higher first ionization energy and higher electron affinity…
Q: Why does potassium have a lower first ionization than lithium ?
A: Electronic configuration of Li : 2,1 Electronic configuration of K : 2,8,8,1
Q: Use the periodic table to arrange the following elements in order of increasing first ionisation…
A: Since the element P and S belong to same period 3 and the element O belong the the period above them…
Q: 8) Arrange affinity (less negative Na,S, and CI the following inorder of increasiing electron tomore…
A: Electron affinity of any element is defined as the amount of energy released when an electron is…
Q: hy fluorin has low electron affinity as compared to chlori
A: When an electron is gained by an atom some energy is released so this released energy is electron…
Q: How many electrons does barium have to give up to hav the same electron configuration as a noble…
A: The electron configuration of an atom is the representation of the arrangement of electrons…
Q: write the formula that corresponds to the definition of electron affinity (EA) of sodium (Na)
A: Electron affinity is the internal atomic factor of the atom .
Q: Based on the table reaction given, 1.Compare the size of O- and O2- . Which of these two ions is…
A: In this question, gievn the compare the size and the electron gain enthalpy of 2nd oxygen , Given…
Q: Sulphur reacts with carbon and potassium separately to form compound P and compound Q. (a) Draw an…
A: Sulfur(S) is more electronegative than both carbon(C) and potassium(K). Hence S accepts electrons…
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- Use the periodic table to arrange the following elements in order of increasing firstionisation energy: P, S, O. Give a brief explanation why you chose this arrangement.For each of the following pairs of atoms, state which youexpect to have the higher electron affinity: (a) Rb or Sr;(b) I or Rn; (c) Ba or Te; (d) Bi or CConsider the isoelectronic series Zr4+, Nb5+, Mo6+, Tc7+. Arrange these species as follows. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) in order of increasing atomic or ionic radius b) in order of increasing ionization energy
- The gadolinium +3 ion (Gd3+) has advantageous magnetic properties for Magnetic Resonance Imaging (MRI) applications, specifically a high number of unpaired electrons. In fact, both neutral Gd and Gd3+ have a set of degenerate orbitals with seven unpaired electrons. a) Write the electron configuration for Gd and Gd3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the +3 cation based on the above information. Explain your reasoning (2-3 sentences). b) Curium (Cm) is an actinide element named for Marie Curie. Cm is in the same group as Gd and also forms a +3 cation. Write the electron configuration for Cm and Cm3+. c) While +3 is the most common oxidation state for lanthanide elements, some can form +2 ions. Identify an isoelectronic ion to Gd3+ that has a +2 oxidation state and indicate which orbitals lose electrons to form that ion.Explain how periodic trends in ionization energy and electron affinity explain why atoms of elements in Group I andGroup II tend to bond with other elements by forming positive ions in ionic compounds. Explain with electronconfiguration of elements belonging to Group I and Group II.How many valence electrons in Groups 1,2,3,5,6,7,8A?
- Write electron configurations of • C, N, O, F, Ne • Be, Mg, Ca • F, Cl, Br • He, Ne, Ar, KrWhy fluorin has low electron affinity as compared to chlorine?2. Explain the following phenomena on the basis of electron configuration. i) Fluorine forms an ion having a charge of -1. Support your answer by providing the electron configuration of both atom and ion. ii) Which is the more likely the configuration for Mn2+: [Ar]4s23d3 or [Ar]3d5. Give reason for your answer.
- Rank the following in increasing order of ionization energy by numbering them in order from 1 through 6, with 1 having the lowest ionization energy and 6 having the highest ionization energy. Se Cr K Br Са KrIn group 15 elements, there is considerable increase in covalent radius from N to P but small increase from As to Bi. Why?In general, ionization energies increase from left to right within a row of the periodic chart. However, oxygen has a lower ionization energy then nitrogen. Еxplain.
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