Which is NOT a characteristi 0luyw5l9l pxl. rdh93c property of metals resulting from metallic bondingll.dx3l5l9ywr 90u h p?

Metallic bonding characterizes;/asbyj*l jw7qkb a- 8 the bonding present in the elemental form of the metals on the periodic table.a/s7q 8-;kbj bj*awly
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 charaq l;dkhy)2u-d e;ha 1ncterized by the following statement:

  Which of the following isaufy3ojh2j/ fvjxi, 3obu:+ e2ir w.1 NOT true of metals?

Properties of substances can be ri ny6x o,i01b35su ofnelated to the type of bonding, including electrical conduo0ni6 yiuofnsb x5 1,3ctivity.
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 indicates, the strength of metallit tv4-2s5y kxp y53clp.u nr4bc bonding?r3yln 5b 5ypt- pkt4sucv.x24

Titanium, lithium, and potassium have m xo(z rvh,l5yj 4cap 5-.pu7vbelting points of 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 series correc 7sl6 ygriz00y ttb66jtly orders the elements by increasing melting poin67zb l00ttgsy 6rj6yits?

  The oxides of two period 3 elements, X and Y, react in0l(4 cum9d kof water according to the equatiok u d04mcl(9fons 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 prop7wr0( xbayr2 certies of the following using knowledge of chemical structure ax0 wcar2yr( 7bnd 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 metallic bonding are corrw8c28xl gqks 9ect?
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 periodiudind/ad )8u3 c table. The group 1 metals react with bromine to form soluble bromide salts, which all have the same ldn8uu ad/ )id3attice 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 followingz ;62rel3yymtcukv sa2 2ld:- are characteristics 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 results in hi:p (w:c0bv+fh4ol9 vnfcnv y4gh electric(49nl0vcv:ynofw fc:+b 4 vhp al conductivity?

  When comparing Ca to Ni, which of the following is tr lv9ho5t, cp8pa78ud hue?

  Vanadium and titanium ar0/ vsjs- c9) ym6gqhfk((tbnx.33if l, cferbe both common metals in aerospace engineering because they 9 sjrgcfhk.m(fb06v,q 3ie c /bl3 -n)x(ytsfhave a high strength to weight 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.