Which is NOT a characteristic property of metals resulting p /-y7-jl4cf0:icyudlfv ,n k from metallic bonding?kl, 7d vljy--:cufin/cp yf04

Metallic bonding characterizes the bonding present in the elemental form ofp43; ql7 ml fu/-mxqhf the metals on the periodic t fl/ ;hmm qqux7p4f-l3able.
1.Describe features of metallic bonding.
2.Describe 3 common properties of metals that result from metallic bonding.
3.Solid sodium chloride is brittle while sodium metal is not. Explain this difference in properties.

  Metallic bonding is best characterized3u w3 )ns8ud18;tnykch. ql si by the following statement:

  Which of the following is NOT true c99/xv4qssg0hq r +y xof metals?

Properties of substances can be related to y lug)*(h1d7hus0 utt the type of bonding, including electrical conducti uydlh)g 1uu(*7ths t0vity.
1.In part (a) of the table below, state examples of one metallic and one non-metallic substance that are electrically conductive.
2.In part (b) of the table below, draw a diagram that demonstrates the bonding of each substance mentioned in part (a).
3.In part (c) of the table below, state why this bonding structure enables electrical conductivity.

Non-metallic Metallic
(a)Substance with electrical conductivity
(b) Diagram or model of structure
(c) Reason for Conductivity

  Which characteristic best corresponds to, or ina5ss fab2jn11u6i4q k +-jozedicates, the strength of metallic b26af b+aeins 1-qk1jj4u z s5oonding?

Titanium, lithium, and potassium have melting points ofuba6ma-br; ; j 1910$^{\circ}C$,181$^{\circ}C$,and 68$^{\circ}C$,respectively.
1.Outline two characteristics of a metallic element that affect the strength of the metallic bond.
2.In terms of atomic structure, the observed melting points of titanium, lithium, and potassium listed above.

  Based on periodic trends, which serieenx7+1dd vt g9s correctly orders the elements by increasing meltind 9n7xde1tvg +g points?

  The oxides of two period 3 elements, X and Y, react in wateev,xhn v( *)gssw,r k4r according to the equat,s (hv*) ervng,4xswkions below.
I. $XO_{2(s})$ + $H_2O_{l}$→$H_2XO_{3(aq)}$
II. $YO_{2(s})$ + $H_2O_{l}$→$Y(OH)_{2(aq)}$
1.Identify elements X and Y. Element X is   ;Element Y is   .
2.Predict whether element X or Y would have a higher melting point. Element  ----待选择----XY  will have a higher melting point than element  ----待选择----XY 

  1.Explain the difference in physical properties 5dwn0h s2ufu3of the following using knowledge of chwds5 un hf032uemical structure and bonding:
.1.The boiling point of hydrochloric acid (HCl) is  ----待选择----lessmore  than that of lithium chloride (LiCl).
.2.Calcium bromide ($CaBr_2$)  ----待选择----cancannot  conduct electricity in a molten state and aqueous solution; Bromine ($Br_2$)  ----待选择----cancannot .
.3.The boiling point of HI is  ----待选择----lowerhigher  than $I_2X$.
2.Arrange bromine ($Br_2$), potassium and potassium bromide in order of increasing boiling points.
 ----待选择----brominepotassiumpotassium bromide ＜ ----待选择----brominepotassiumpotassium bromide ＜ ----待选择----brominepotassiumpotassium bromide 

  Which statements regarding myuse38( m0f, a eub4gbo0- ceretallic bonding are correct?
I.The higher the charge on the ion of a metallic element, the weaker the bond
II.A metallic element with a greater ionic radius will have a weaker metallic bonding
III.Metallic bond strength increases with the number of delocalized electrons

Lithium is a metal in group 1 of the periodic table. The group 1 m4 v;sax,7pq hdetals react with bromine to form soluble bromide salts, which all have the same lattice p, d7h;4qvaxs structure.
1.The melting points of the group 1 metals and their bromide salts are shown in the graph.


1.Explain the variation in the melting points of the group 1 metals.

2.The following diagram shows the electron density distributions formed when bromide ions interact with lithium and sodium ions.

Based on the diagram, suggest why the melting point of lithium bromide is lower than that of sodium bromide.
2.Lithium is a good electrical conductor, whereas lithium bromide is an electrical insulator.
.1.Explain the difference in the electrical conductivities of lithium and its bromide salt.
.2.Explain how water interacts with lithium bromide to produce an electrically conductive solution.

  Which of the following are characteristicssjv .v++gc/z*rk mg k: of transition elements?
I.High melting points
II.Soft
III.Electrically conductive

  Which of the following explains why transition metals have high melting points?

  Which of the following characteristics of transition metals results7n+ z + cbtfbs4m8ld+pbq2l, s in high electrical conductivityb d4tlsq2 bf8z+ s+c7n,+bpml?

  When comparing Ca to Ni, which of the following i(9uzdq kxhes4 54fv; 8ai +vkgs true?

  Vanadium and titanium are both ckq d0gbwdbq; wx t7b1g +t;3er8( wb7kommon metals in aerospace engineering because they have a high strength to wq7 d+qw; x(b3 r7 w1tgb; dkgktwe0b8beight ratio.
1.vanadium has a  ----待选择----higherlower  melting point than titanium.
2.Titanium and vanadium are both able to conduct electricity. Explain how this is possible.
3.Tin is not a good choice for use in aerospace engineering. Predict, with a reason, why this is so.