Which is NOT a characteristic property of metals resulting from metallic bondh 9zotti:l90v ing?itl zv o90ht9:

Metallic bonding characterizes the bonding prvamh4wt;+o6ce yp3f+j7 p7e szbb .k9esent in the elemental form of the metals on t+4cp.37v; oajmsetb eb 9yzhf6+kp7 whe periodic 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 charal7qc64i-y. wdodtj *i cterized by the following statement:

  Which of the followinljll t-q unr:) fbmen e(gd o5.v3b+56g is NOT true of metals?

Properties of substances can be related to the type of bon hgf: mgr-;8dhding, including electrical condum:fghd ; gr-8hctivity.
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 vimetq)5* fvo3s;7 7cis9ahkto, or indicates, the strength of metallic bondina5fk7v 9);q 3sv ieci so*hmt7g?

Titanium, lithium, and potassium have m -z5g u4pe:*jw- oqxqgelting 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 thoiub y: giu*aau wp7n45* ,3rhe elements by increasing melting po un*ab,wioayug4:p75 * hr 3iuints?

  The oxides of two period 3 elements, X andc .r(uxruf;w; t49wlb/bs *jc Y, react in water according to the eq/us9. w4 (jbwt* r;cbruf cl;xuations 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 phystinp/fq 86.fzjg vv52 ical properties of the following using knowledge of chemical stnfv/58 6t v qp.i2zjfgructure 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 metallic (3smfg sa vzn)aw76 ofy( 01ftbonding 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 os id1 gku-nrr x0x9p35f the periodic table. The group 1 metals react with bromine to form soluble bromide salts, wh-1rx0ug3ndxs95 ri pkich 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 chara-p ;r u(clsfdwf5 :dh7r/;ok gcteristics 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 trk;m3c. 9biwg, yc)xxe ansition metals results in high elecb9) .,; ekgi3xymccx wtrical conductivity?

  When comparing Ca to Ni, whic vh6nf(q1ug.sh of the following is true?

  Vanadium and titanium are botqmkhb vaox d -8h)vv k(au8ju 7p2u5(7h common metals in aerospace engineering because they have a high strength to weu(d8vu vhbvp uxk(oqa h-7)872akm 5jight 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.