Which is NOT a characteristic property of metals resulting from me52amd4 nj9 basp(ym6vtallic bondingvpb5( d62as yam9jmn 4?

Metallic bonding characterizy.pu;gld 49pd es the bonding present in the elemental form of the metals on the pg. p4dd l;yp9ueriodic 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 g,mel0 k,rs 7hfsh:h) characterized by the following statement:

  Which of the following is NOT true of metals?eiy u(;o bsb+/

Properties of substances u hxugfs(cl i)54c)a1 can be related to the type of bonding, including electrical cond(5)s)lc4hu1 f igauxcuctivity.
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 corf xiqga+y(/ 4lresponds to, or indicates, the strength of metallic bondinq x (fiya4gl+/g?

Titanium, lithium, and potassium have melting points of 1916) lh,ube4ecp 0$^{\circ}C$,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 elemion g,h0. 1jvw1 e2r6bukh(xtojg11x ents by increasing bgok1 .( rj,v21i e01hownux1xh6tjg melting points?

  The oxides of two period 3 elements, X and Y, react in water accorqpf,f c cz67npay;i: ;4(, ihj1eepfcding to the equf4y 71qh ncec, e6facj;:,fi pi( ;pzpations 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 ofx9cn mxskq:1gidzim 3m5b4 3 k.eth93 the following using knowledge of chemical structure ae4qmi kx5mkt3xdn1.3i:3 9 bhg z9cm snd 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 me(u59wk-tb rawfey/ 5qtallic 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 1 of the periodic table. The group9wg f/h3tx b2m4 pqtb7 1 metals react with bromine to form soluble bromide salts, which alb7 xm/p 23t4g9fwqhbtl 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 charactekgv r skt+).s-ristics 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 high elq7 vo )bhn8gd c0bnc h4b a4o06mfo,e y3tr,m0ectrv4q00)4a6yfh dbg8t7ccmrn nmb0o 3ehb ,o,oical conductivity?

  When comparing Ca to Ni, which of the followinge6n f ehp/-p,g is true?

  Vanadium and titanium are b2.ox 8diz .dz (h)1n xfaz5wiioth common metals in aerospace engineering because they have a high strengzna1x(idwd zoh i..) 5x82fzi th 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.