(a)
Interpretation:
The noble gas having identical configuration to
Concept introduction:
A representation of filling of electrons in orbitals in a systematic manner is known as electronic configuration. The pattern of filling of electrons is based on three principles that are Aufbau’s principle, Pauli-exclusion principle, and Hund’s rule.
(b)
Interpretation:
The noble gas having identical configuration to
Concept introduction:
A representation of filling of electrons in orbitals in a systematic manner is known as electronic configuration. The pattern of filling of electrons is based on three principles that are Aufbau’s principle, Pauli-exclusion principle, and Hund’s rule.
(c)
Interpretation:
The noble gas having identical configuration to
Concept introduction:
A representation of filling of electrons in orbitals in a systematic manner is known as electronic configuration. The pattern of filling of electrons is based on three principles that are Aufbau’s principle, Pauli-exclusion principle, and Hund’s rule.
(d)
Interpretation:
The noble gas having identical configuration to
Concept introduction:
A representation of filling of electrons in orbitals in a systematic manner is known as electronic configuration. The pattern of filling of electrons is based on three principles that are Aufbau’s principle, Pauli-exclusion principle, and Hund’s rule.
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Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Which of the following statements are true regarding a covalent bond between nitrogen and oxygen atoms in a nitric oxide, NO, molecule? (a) Valence electrons are shared between nitrogen and oxygen atoms. (b) Bonding electrons are found only between the bonded atoms. (c) The bond length is greater than the sum of the two atomic radii. (d) Energy is required to break a covalent bond.arrow_forwardQuestion Five Use the periodic table provided and answer the following questions: (a) Cesium Bromide (CsBr) exhibits predominantly ionic bonding. Cesium (Cs) has an atomic number of 55 while Bromine (Br) has an atomic number of 35. State the following: (i) The electron configuration for the Cesium ion (Cs") and the Bromine ion (Br). (ii) Which inert gases can the two ions above be associated to? (b) Describe fully how an ionic bond is formed. (c) Given that radioactive cobalt-60 has a radioactive constant equal to 7.6 x 10° s', determine its half- life and how long would it take for the activity of a sample of cobalt-60 to reduce to 20 % of its original value ?arrow_forwardWhich of the following elements does not follow the octet rule? (a) sodium (b) helium (c) krypton (d) carbon (e) sulfurarrow_forward
- Na+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardThe atomic number of sulfur is 16. Sulfur combines withhydrogen by covalent bonding to form a compound, hydrogensulfide. Based on the number of valence electrons in a sulfuratom, predict the molecular formula of the compound.(A) HS(B) HS2(C) H2S(D) H4Sarrow_forwardAnswer true or false. (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency of certain elements to react in such a way that they achieve an outer shell of eight valence electrons. (c) In gaining electrons, an atom becomes a positively charged ion called a cation. (d) When an atom forms an ion, only the number of valence electrons changes; the number of protons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of 12. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one electron to fill its 3s shell (1s22s22p63s2). (g) The elements of Group 6A typically react by ac- cepting two electrons to become anions with a charge of 22. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1, 2, and 3. (i) Atoms and the ions derived from…arrow_forward
- Write an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ararrow_forwardWrite the chemical formulas for the following compounds:(a) Silver cyanide(b) Calcium hypochlorite(c) Potassium chromate(d) Gallium oxide(e) Potassium superoxide(f) Barium hydrogen carbonatearrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (The ionic compound as a whole, not just OCN-) (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forward
- Which statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table . (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forwardHow many electrons are in the valence shell of each atom? (a) Carbon (b) Nitrogen (c) Chlorine (d) Aluminumarrow_forwardPredict which ions are stable: (a) Br2- (b) C4- (c) Ca+ (d) Ar+ (e) Na+ (f) Cs+arrow_forward
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