Which is NOT a character3kvd3* 4wcwx0(bh)ysef:e m mistic property of metals resulting from metallic bonding?43w:(e yfsdhcx0vmbe3kw* m)

Metallic bonding characterizes the bonding present in the elemental formbu x+8 s;)tdjpla9lb , of the metals on the periodic tablebt+d la, u)8l;9xjb sp.
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 characterized b2m9ox te:g5g5 ew(q+ey) excp y the following statement:

  Which of the following is u .we6 e p.woye;jq/*rNOT true of metals?

Properties of substances can be related to the type of ;tp ,ew m.(tzfbonding, including electrical condz.(em,wtp ;f tuctivity.
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 to3 r4ig z(pibfu*5 e8flpc1 k6h, or indicates, the strength of metallic bonding?8b*fi zplfg43e(ip 1u5k 6c hr

Titanium, lithium, and potassium have meli( 5ft.8 9wsqdjt8nxlxt 04svo/a5d rting 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 corj5p cnvv8n3 h1rectly orders the elements by increasing melting poinv3 n18jc5pvh nts?

  The oxides of two period 3 elements, X and Y, react in zukjm s8-y , 6oxpwnh ,z93vb1water according to the equationsj sno,mz-b,vpxu w8k9316hzy 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 mak6dj x31kg ;in physical properties of the following using knowledge of chemical kjx ;63d g1kmastructure 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 regardig nyu k.+u:0qjng metallic 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 1u,*y 7ldz.q:k xs*ttj of the periodic table. The group 1 metals react with bromine to form soluble bromide salts, which all have the same lattice structkq*u s j7z*l dt,:y.txure.
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 characteristics q7xh3nua+;mih1dsge*cf m (6y* c d1gof 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 transi0wl6x do2)*(gx,ri gauc ss5 ition metals results in high electrical conduct6x2 0rgsgcdouli , a)w5x*i(sivity?

  When comparing Ca to Ni, which o4nzc4lj jjrz,k)l a,/8r oox q*aq *7kf the following is true?

  Vanadium and titanium are both common metals in aerospace engineering because 2f+) *3xl bvh boy*vfkthey have a high strength to weight*bf3 kxy)o+vh2lf * bv 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.