Which is NOT a characteristic proper *d;nb40xwu hqty of metals resulting from metallic bondingd*40hqnb;x u w?

Metallic bonding characterizes the bonding prese/lxl m( wk,y)knt in the elemental form of the metals on the periodi/ klk xy,()lmwc table.
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 characterige -/sy/st ;,ra kybiod::4a ized by the following statement:

  Which of the followinhuw z7w;n2glu62c 416omxnjk /t/e g9 6djdaog is NOT true of metals?

Properties of substances can be relat2bq(j.2qe z jned to the type of bonding, including electri qz2jebn2 q(j.cal conductivity.
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 stre5k :/qhcrh:c sngth of metallic bondhkqc cr/ :s:h5ing?

Titanium, lithium, and potassium have meltinoglh9e bm06,hg 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, whico0fupwy 51e/ -j.uh heh series correctly orders the elements by increasing y .0 -5 hofe/ueujph1wmelting points?

  The oxides of two period 3 elements, X and Y, react in water according in /g)ig0h6cr-5iz y qp9d+ czto the equations cq/iiz rig9pg6 )czn0h+5-d y 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 of th 6xke4n6d ncg5o fos wv+(ueb*2d1u m,e following using knowledge of chemical structure and bondi6b,(4u w ok odxueems 5*1vnf nc+gd62ng:
.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 correox++ynab-.v ict?
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 gr 5x(sie95u-fe)pr xh roup 1 metals react with br -u) if9r55( xhpsrexeomine to form soluble bromide salts, which all have the same lattice 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 c7lk;i ,*) zoo.b3pnz:si zpzrharacteristics 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 characlbzqwo6qul8 ;5hl (; steristics of transition metals results in high elecl l6hs ;zw8q (oubql;5trical conductivity?

  When comparing Ca to Ni, whg**rtb7qi1rz:ovqn v:m- x r0m( ce a1ich of the following is true?

  Vanadium and titanium aqh+)1ecz4cw7:sfv lg re both common metals in aerospace engineering because thh4:+ s1qfz7e v clc)gwey have 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.