Q: Electron affinity - from left to right within a period from top to and _-- bottom within a group. O…
A:
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…
A:
Q: Consider the isoelectronic series Zr4+, Nb5+, Mo6+, Tc7+. Arrange these species as follows. (Use the…
A:
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…
A:
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?
A:
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…
A:
Q: What are the identidication tests used for the group III and IV elements? Give comprehensive…
A:
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…
The second
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- Hydrogen is an unusual element because it behaves in someways like the alkali metal elements and in other ways likenonmetals. Its properties can be explained in part by its electronconfiguration and by the values for its ionization energyand electron affinity. (a) Explain why the electron affinity ofhydrogen is much closer to the values for the alkali elementsthan for the halogens. (b) Is the following statement true?“Hydrogen has the smallest bonding atomic radius of anyelement that forms chemical compounds.” If not, correct it.If it is, explain in terms of electron configurations. (c) Explainwhy the ionization energy of hydrogen is closer to the valuesfor the halogens than for the alkali metals. (d) The hydrideion is H-. Write out the process corresponding to the firstionization energy of the hydride ion. (e) How does the processin part (d) compare to the process for the electron affinityof a neutral hydrogen atom?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 C
- Consider 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 energyHow many valence electrons in Groups 1,2,3,5,6,7,8A?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.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?
- 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 Kr2. 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.In group 15 elements, there is considerable increase in covalent radius from N to P but small increase from As to Bi. Why?