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(a)
Interpretation:
Whether the valence electrons are more, fewer or the same for first element compared to the second one in the following pair -
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- Except inner
transition elements valence electrons are present in s or p subshells of elements. - For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
The ways in which electrons are arranged into various orbitals around the nuclei of atoms is called electronic configuration.
(b)
Interpretation:
Whether the valence electrons are more, few or same for first element compared to the second one in the following pair -
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- Except inner transition elements valence electrons are present in s or p subshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
The ways in which electrons are arranged into various orbitals around the nuclei of atoms is called electronic configuration.
(c)
Interpretation:
Whether the valence electrons are more, few or same for first element compared to the second one in the following pair-
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- Except inner transition elements valence electrons are present in s or p subshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
The ways in which electrons are arranged into various orbitals around the nuclei of atoms is called electronic configuration.
(d)
Interpretation:
Whether the valence electrons are more, few or same for first element compared to the second one in the following pair-
Concept Introduction:
The electrons present in the outermost shell of the atom are known as valence electrons.
Valence electrons are important because:
- The valence electrons decide the reactivity of an element.
- Except inner transition elements valence electrons are present in s or p subshells of elements.
- For inner transition elements incompletely filled d or f subshells electrons are considered as valence electrons.
- The group number is similar to number of valence electrons of an atom.
The ways in which electrons are arranged into various orbitals around the nuclei of atoms is called electronic configuration.
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Chapter 4 Solutions
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
- What are bus? How are ions formed from atoms? Do isolated atoms form ions spontaneously? To what do the termscationandanionrefer? In terms of subatomic particles, how is an ion related to the atom from which it is formed? Does the nucleus of an atom change when the atom is converted into an ion? How can the periodic table be used to predict what ion an element’s atoms will form?arrow_forwardHow many valence electrons are needed to complete the outer valence shell of sulfur? a. 1 b. 2 c. 3 d. 4arrow_forwardFor each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ioncontains. A given answer may be used more than once. Column 1 Column 2 [ 1] Se2 [a] 18 [ 21 S2 [b] 35 [ 31 P3 [c] 52 [ 4] O2 [d] 34 [ 5] N3 [e]36 [6] I [f] 54 [7] F [g] 10 [8] Cl [h]9 [9] Br [i] 53 [101 At [j] 86arrow_forward
- An element X reacts with hydrogen to form a compound of formula HX. In which group in the periodic table is X most likely to be found? a. 1A b. 2A c. 7A d. 8Aarrow_forwardIndicate the number of electrons lost or gained when each of the following atoms forms an ion. a. 37RB b. 53I c. 8O d. 11Naarrow_forwardGive the symbol of four stable ions formed from Main Group elements that are isoelectronic with Argon. d. a. b. с.arrow_forward
- Which will form an ion with a +2 charge?A. S B. Br C. Ba D. Csarrow_forward1. The higher the number of electrons in an atom, the higher the effective nuclear charge will be. - True - False 2.The Bohr atomic model states that electrons move from one orbit to another orbit when they absorb or emit photons - True - False 3. Which of the following compounds is a possible combination of a metal and nonmetal taking into account their stable ions? a.NaI2 b.CaF3 c.MgBr d.Al2S3 4. Which of the following compounds has contains the strongest bond? a.CH4 b.C2H2 c.C2H4 d.CH3Clarrow_forwardDefine the term main group element. Then, determine the charge that an atom of each of the following elements will normally have when it forms an ion. a. sodium b. bromine c. aluminum d. sulfur e. bariumarrow_forward
- Predict the charge of the ion most likely to form for each.a. F b. Sr c. Group VA d. The Noble Gasesarrow_forwardHow many valence electrons do the atoms of the following elements contain? 4 valence electrons 1. S 2 valence electrons 2. Ra 6 valence electrons 3. Rb 1 valence electrons 4. Si 5. Xe 8 valence electrons 18 F2 F3 O00 F4 II F5arrow_forwardCHEMISTRY 101 LECTURE NOTES 4. Give one example (atomic symbol and name) for each of the following. a. a main-group (representative) element in the second period b. an alkali metal c. a transition element in the fourth-period d. a lanthanide element 5. Write the formula for the compound of each of the following pairs of ions. a. Fe and CN b. K' and SO,² c. Li' and N³ d. Ca²² and P e. NH, and PO, 6. The following table gives numbers of electrons, protons, and neutrons in atoms or ions of a number of elements. Answer the following: (a) Which of the species are neutral? (b) Which are negatively charged? (c) Which are positively charged? (d) What are the conventional symbols for all the species? Atom or lon of Elenment B Number of electrons 10 18 28 Number of protons Number of neutrons 36 5. フ 19 30 35 20 36 46 7. Consider a hypothetical case in which the charge on a proton is twice that of an electron. Using this hypothetical case, and the fact that atoms maintain a charge of 0, how many…arrow_forward
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