Which is NOT a characteristic property of metals rvepitd04 )m i.esulting from metallic bondingimit.vpd04e )?

Metallic bonding characterizes the bonding stk+:o2li+uz present in the elemental form of the metals on the periu l2+os+ki:z todic 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 be13id; h3zbcdh un-j/ tst characterized by the following statement:

  Which of the following is NOT true of m4towq0,9m ju qetals?

Properties of substances can be related to the type of bondi1unb0l rg8t)sb0qm h,-s kye; ng, including electrical conductivi8bh ;00-g)1ktusm rs ebnq,ylty.
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 metallic8xbjp+j2o *w e bonjb pxwo j8*e2+ding?

Titanium, lithium, and potassium have meltd-aq.- ;qei( oi( ptkoing 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 correctly orders the elem-l ycng 99gk1h5wii-+iz( fpnents by increasing k-9wg yi-1i+ipzcng( n9lhf5melting points?

  The oxides of two period 3 elements0g/a1hyb(zoa , X and Y, react in water according to the equations below.y(g/0h b1zoa a
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 propertmh2 4yk bfcdz;(+ sski ig/31mies of the following using knowledge of chemical structure and bondin +f skby3zmsh 2gckd ;(4mi/1ig:
.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 o*va tq:fu , ge:o;b*qare 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 peri+qi h*s fmd84sz;zy5sz oqehi o*+8 (bodic table. The group 1 metals react with8z4qfqdsoz ;o+ 58hz m+*sb seiy*i (h bromine 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 characteristic2 f/ic0iy w1 jiu2v)hns 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 cha; kxiquyae*m uu.yh,n, (gun8 (0o1 cfracteristics of transition metals results in high elec,0ucg8( ; 1xonu ay*uk,yuihe. qfm (ntrical conductivity?

  When comparing Ca to Ni, whifuk1,ve c :jvacyf :vu w6( 0m+lnnz0-ch of the following is true?

  Vanadium and titanium are both common metals in aerospace engineerin cv904 9tiap :bj)xw hsbxbe80pm)z 0sg because they have a high strength to weight rat8w0)s jsmppzb0eb):90atxchv x i 94b io.
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.