7.83 Referring to the periodic table, name (a) the halogen inthe fourth period, (b) an element similar to phosphorusin chemical properties, (c) the most reactive metal in thefifth period, (d) an element that has an atomic numbersmaller than 20 and is similar to strontium.
Q: 7.3 A Referring only to a periodic table, arrange the elements Ge, Se, and F in order of increasing…
A: To find: The increasing order of atomic radius for the given elements
Q: A main group element with the valence electron configuration 2s22p3 is in periodic group__________…
A: Given electronic configuration is 2s22p3
Q: 6 The elements of the Periodic Table are created by a variety of processes discussed in the…
A: New atomic nuclei create from pre existing nucleons.The first nuclei form after bing bang through…
Q: Which halogen has the highest ionization energy? Explain why.
A: Hi, since you have posted multiple questions. We will answer the first questions. Kindly repost the…
Q: 7.85 Arrange the following isoelectronic species in order ofincreasing ionization energy: O2−, F−,…
A: Arrange the following isoelectronic species in order of increasing ionization energy: O2−, F−, Na+,…
Q: Explain why the s-block of the periodic table is twogroupswide, the p-block is six-groups wide, and…
A: The reason why s-block of periodic table is two groups wide, p-block is six-groups wide and d-block…
Q: Choose the most correct statement about atomic and ion radius. O a) The radius of a metal ion is…
A: Given : We have to choose the correct statement.
Q: Mention 3 general characteristics of the s-block elements that distinguishes them from the other…
A:
Q: 7.36 Which is the largest atom in the third period of the periodic table?
A: In periodic table, there are total 7 periods (along horizontally), 18 groups (along vertically), and…
Q: Which has the larger radius, S or S2-? Explain.
A: Which has the larger radius, S or S2- has to be identified.
Q: Tungsten has the highest melting point of any metal in theperiodic table: 3422 °C. The distance…
A:
Q: how can you be reasonably sure that arranging elements by their atomic number is accurate?
A:
Q: 7.72 Give the physical states (gas, liquid, or solid) of themain group elements in the fourth period…
A: Intermolecular forces refer to the type of interactions which are present in between atoms or…
Q: How does the ionic radius of a nonmetal compare withits atomic radius? Explain the change in radius.
A: The atomic radius is the distance between the nucleus and the outermost shell of the element. On the…
Q: Rank the following in increasing order of atomic size (atomic radius) by numbering them in order…
A: Electronic configuration of Be: [He] 2s2 Electronic configuration of Mg: [Ne] 3s2 Electronic…
Q: A main group element with the valence electron configuration 4s24p4 is in periodic group ______ .It…
A: The outer electronic configuration of the element is 4s2 4p4. This implies that it has 6 electrons…
Q: 7.45 In general, the first ionization energy increases from left to right across a given period.…
A: Magnesium and aluminum lies in the same period - 3 but in different groups. Magnesium is the block…
Q: A. A main group element with the valence electron configuration 3s1 is in periodic group? It forms a…
A: According to octet rule, a element or ion is stable enough when it has its octet completed. i.e. 8…
Q: Arrange the following groups of atoms in order of increasing size. Beginning with the smallest and…
A: The neutral element have more radius than cation form of same element because cation is formed on…
Q: 3. Write down the equation of the highest ionization energy of Sulfur (S) and explain why it is the…
A: Ne3S23P4→Ne+6e-
Q: exceptions to the periodic trends in ionization energy?
A: Normal trend ; Ionisation energy increases down the group ,due to increases in atomic size and…
Q: Rank the following in increasing order of ionization energy by numbering them in order from 1…
A:
Q: 8.48 (a) Why do successive IEs of a given element always in- crease? (b) When the difference between…
A: Ionisation energy is the amount of energy required to remove electron from an isolated gaseous atom.…
Q: Describe the relationship between:a. the radius of a cation and the radius of the atom from which it…
A: a) When the electrons are lost from an atom, it leads to the formation of a cation. This results in…
Q: 3. Relative Atomic Sizes. Rank the following in increasing order of atomic size (atomic radius) by…
A: On moving from left to right in a period atomic size decreases. This is because of the increment in…
Q: 7.127 Explain why it is more difficult to ionize a fluorine atom than a boron atom.
A: Answer
Q: Describe 2 reasons the C atom is unique separate when compared to the elements closest in one period…
A: A question based on Carbon atom, which is to be accomplished.
Q: What is the difference between ionic radius and atomic size?
A: An atom is a neutral species while an ion is a charged species. An ion can be positively or…
Q: Arrange the following in order of increasing ionization energy: P, Ca, Cs, Ge, O, Ba
A: Ionization energy: It defined as the minimum amount of energy required to remove the most loosely…
Q: Of the elements Li, K, N, P, and Ne, which has the greatest metallic character?
A: Metallic character of the elements increases down the group and decreases along the period from left…
Q: d) Suggest a reason for 5. a) Explain the term periodic trend when applied to trends in the periodic…
A: Periodic patterns, which arise from the periodic table's arrangement, provide chemists with a…
Q: 4. Which element has the greatest electron affinity?
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: (2) The element with an electron configuration of 1s22s22p63s2 is in group ______and period ____.
A: Electron configuration of Magnesium:
Q: for the element being described in each of the following. (Hint: Use the Periodic Table of Elements…
A: In a group of periodic table atomic radius increases , when we move from up to down. In a period of…
Q: separate
A: This question is related to periodic table.
Q: A. A main group element with the valence electron configuration 35 is in periodic group 2 It forms a…
A: Answer for A.: Mg, +2 Answer for B.: Se, -2
Q: Moseley’s experiments on X rays emitted from atoms led tothe concept of atomic numbers. (a) If…
A: a. Now to see which element is placed next to chlorine in the order of increasign atomic mass we…
Q: As we move across a period of the periodic table, why dothe sizes of the transition elements change…
A: The reason is as given below;
Q: 5. Placed the elements N, O, As, Se in order from least to greatest atomic radius. a. N<0<As < Se b.…
A: The question is based on the periodicity of elements. we have to arrange the given atoms in…
Q: name of the element with the largest atomic radius in Period 6
A:
Q: What is meant by first ionization energy" Using calcium as an example, write a ba ionization energy.…
A: An atom is the smallest unit of matter that forms a chemical element and an atom takes part in a…
Q: Knowing that atomic radius and ionization energy are two important properties of an atom that are…
A: Atomic radius : It is the distance measured from the centre of nucleus to the outermost electron .
Q: The elements of a period in the periodic table are given below in order from left to right: 3li „Be…
A: The period of the given set of elements have to identified and the one which has larger atomic…
7.83 Referring to the periodic table, name (a) the halogen in
the fourth period, (b) an element similar to phosphorus
in chemical properties, (c) the most reactive metal in the
fifth period, (d) an element that has an
smaller than 20 and is similar to strontium.
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- Arrange in order of increasing nonmetallic character. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 4 elements V, Ge, and K (b) the Group 5A elements N, As, and Bi Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 3 elements Mg, Si, and Ar (b) the Group 2A elements Ca, Ba, and SrQ2. This question is about the periodicity of the Period 3 elements. (a) State and explain the general trend in first ionisation energy across Period 3. Give one example of an element which deviates from the general trend in first (b) ionisation energy across Period 3. Explain why this deviation occurs. Page 3 of 12 (c) The table shows successive ionisation energies of an element Y in Period 3. lonisation number 1 2 3 4 5 6 7 8 lonisation energy kJ mol- 1000 2260 3390 4540 6990 8490 27 100 31 700 Identify element Y Explain your answer using data from the table. (d) Identify the Period 3 element that has the highest melting point. Explain your answer by reference to structure and bonding.( a ) Eva l u a te t h e expre s s i o n s 2 * 1, 2 * 11 + 32,2 * 11 + 3 + 52, and 2 * 11 + 3 + 5 + 72. (b) How do the atomic numbers of the noble gases relate to the numbersfrom part (a)? (c) What topic discussed in Chapter 6 is thesource of the number “2” in the expressions in part (a)?
- Identify the true statements concerning the atoms andions of the group 6A elements. (a) The ionic radii are larger than the atomic radii becausethe ions have more electrons than their correspondingatoms.(b) Atomic radii increase going down the group because ofincreasing nuclear charge.(c) The ionic radii increase going down the group becauseof the increase in the principal quantum number ofoutermost electrons.(d) Of these ions, Se2- is the strongest base in water becauseit is largest.Q1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic massArrange in order of increasing atomic size. (a) the period 3 elements Cl, Na, and Ar (b) the Group 2A elements Ca, Be, and Mg
- Until the early 1960s, the group 8A elements were calledthe inert gases. (a) Why was the term inert gases dropped?(b) What discovery triggered this change in name? (c) Whatname is applied to the group now?choose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricityThe graph at the right shows the atomic radius for the19 elements in the periodic table.(a) Describe the trend in atomic radius in going fromH (atomic number 1) to K (atomic number 19).(b) Find the three elements represented with blue dotson a periodic table. What do their placements in thetable have in common?(c) Find the three elements represented with red dotson a periodic table. What do their placements in thetable have in common?(d) Based on the graph, what is the radius of C?
- a ) Eva l u a te t h e expre s s i o n s 2 x 1, 2 x (1 + 3),2 x(1 + 3 + 5), and 2 x (1 + 3 + 5 + 7). (b) How do the atomic numbers of the noble gases relate to the numbersfrom part (a)? (c) What topic discussed is thesource of the number “2” in the expressions in part (a)?vi. Answer true or false. (a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration. (b) All Group 1A elements have one electron in their valence shell. (c) All Group 6A elements have six electrons in their valence shell. (d) All Group 8A elements have eight electrons in their valence shell. (e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth. (1) Period 2 results from filling the 2s and 2p orbitals and, therefore, there are eight elements in period 2. (g) Period 3 results from filling the 3s, 3p, and 3d orbitals and, therefore, there are nine elements in period 3. (h) The main-group elements are s block and p block elements.1. An element has the following electronic configuration: [Kr]4d105s25p4(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element? 3. (a) Which of the following atoms or ions is diamagnetic?Li+ Ni2+ Al Fe2+ Mn3+(b) Which of the following atoms or ions is paramagnetic?C4- S4+ V4+ Se2- Ge4+