answer : A METALLIC,In a metal, the outermost electrons, which are known as valence electrons, are not strongly held by individual atoms but are free to move throughout the entire metal lattice. These valence electrons are sometimes referred to as "metallic electrons. " They are not bound to any specific atom and are delocalized, forming a shared "sea" of electrons that move freely within the crystal lattice of the metal. This mobility of electrons is what allows metals to conduct electricity so effectively, as the free electrons can carry an electrical current. 50
12. In general, what can be said of the melting points of metals? a. They are low. b. They are high. c. They are lower than nonmetals. d. They do not have melting points. 51
answer : b They are high,Metals typically have high melting points compared to many other substances. This high melting point is a consequence of the strong metallic bonds that hold the metal atoms together in a regular lattice structure. 52
13. I can hit a metal with a hammer without the metal shattering because of its __________. a. Ductility b. Malleability c. Conductivity d. Lustrousness 53
answer : b Malleability is a property of metals that allows them to be hammered or rolled into thin sheets without breaking or shattering. This property is a result of the metallic bonding and the ability of metal atoms to slide past one another when a force is applied. The delocalized electrons in the metallic bond allow the metal atoms to maintain their structural integrity even when subjected to deformation. 54
14. Metals like to ________ electrons. a. Gain b. Lose c. Anhilate d. Juggle 55
answer : b Lose,Metals tend to lose electrons to achieve a stable electron configuration. This is because most metals are located on the left side of the periodic table (Groups 1 and 2, and the transition metals), and they have relatively few electrons in their outermost energy levels (valence electrons). By losing these valence electrons, metals can achieve a full or nearly full outer electron shell, which is a more stable and lower-energy configuration. 56
15. There are more metals than non metals in the periodic table. a. True B. False 57
answer : a True,there are 89 metals and 22 non-metals 58
16. What do metals conduct? a. heat b. electricity c. both d. neither 59
answer : c both,Metals are excellent conductors of both heat and electricity due to their unique properties. This conductivity is a result of the metallic bonding and the presence of delocalized electrons within the metal lattice. 60
17. What does malleable mean? a. able to be shaped b. will break easily c. can be used for wire d. is shiny 61
aNSWER : A able to be shaped,Malleability is a physical property that describes the ability of a material, typically a metal, to be easily deformed or shaped by applying compressive forces, such as hammering, rolling, or pressing, without breaking or fracturing. In other words, a malleable material can be flattened into thin sheets or molded into various forms without losing its structural integrity. 62
18. Why are alloys generally used to make everyday objects? a. Alloys are often stronger and less active than pure metals. b. Alloys have higher melting point than pure metals. c. Alloys are less expensive to produce than pure metals. d. Alloys have ionic bonds instead of metallic bonds. 63
answer : a Alloys are often stronger and less active than pure metals.Alloys are generally used to make everyday objects for several reasons, but the primary reason is that alloys often exhibit improved properties compared to pure metals. 64
19. Metallic bonding is... a. a type of covalent bond. b. a type of ionic bond. c. an attraction between positive and negative ions. d. an attraction between positive ions and electrons. 65
ANSWER : D an attraction between positive ions and electrons.The positively charged metal ions (cations) are located within this electron sea. The attraction between these positively charged metal ions and the negatively charged free electrons is what constitutes metallic bonding. It's important to note that metallic bonding is distinct from covalent bonds (answer a), ionic bonds (answer b), and the attraction between positive and negative ions (answer c) which are characteristic of other types of chemical bonding in different materials. 66
20. Why do metals conduct electricity? a. They are shiny b. The electrons are held tightly within the lattice c. The electrons are delocalised and able to move d. The electrons are shared between two metal ions 67
ANSWER : C The electrons are delocalised and able to move,Metals have a unique type of bonding called metallic bonding. In metallic bonding, the outermost electrons of metal atoms are not tightly bound to individual atoms but are delocalized, meaning they can move freely throughout the entire metal lattice. These delocalized electrons are shared by all the metal atoms, creating a "sea" of free electrons that can move when a voltage is applied. 68
21. when one atom transfers one or more valence electrons to another atom, a(n) __________ is formed. a. covalent bond b. IONIC BOND C. METALIC BOND 69
ANSWER : B that result from the exchange of one or more valence electrons from one atom, typically a metal, to another, typically a nonmetal. This electron exchange results in an electrostatic attraction between the two atoms called an ionic bond. 70
22. In general, bonds between a metal and a nonmetal are A. COVALENT B. IONIC C. METALIC 71
ANSWER : B IONIC BONDING involves the transfer of electrons from a metal atom to a non-metal atom until the outer shells of their resultant atoms are similar to that of a noble gas. 72
23. When forming bonds, metals tend to A. GAIN ELECTRONS B. LOSE ELECTRONS C. LOSE PROTONS 73
answer : b In a reaction between metals and nonmetals, metals generally lose electrons to complete their octet and non-metals gain electrons to complete their octet. Metal atoms lose electrons from their outer shell when they form ions: the ions are positive, because they have more protons than electrons. 74
A. two atoms that are sharing electrons to complete their respective octets B. two atoms that independently have full octets C. two atoms that independently have full octets 24. An ionic bond forms between 75
answer : c Ionic bonding is the attraction between positivelyand negatively-charged ions. These oppositely charged ions attract each other to form ionic networks (or lattices). Electrostatics explains why this happens: opposite charges attract and like charges repel. 76
25. Electrostatic attraction occurs between A. TWO NEutral atoms B. TWO ATOMS OF Opposite charge C. two positive ions 77
answer : b It is defined as the force between the electrical charges of unlike polarity present in the different atomic proximity. It is always directed towards the center of the ionic bond along the line. This line is also called the internuclear axis, joining the two attracting entities. 78
26. Positive ions are called A. anions B. cations C. dogions 79
answer : b Cations are the positively charged ions and are formed by the loss of electron(s). 80
27. An anion has a __________ charge. A. NEGATIVE B. POSITIVE C. NEUTRAL 81
answer : a Anions are the negatively charged ions and are formed by the gain of electron(s) 82
28. Any halogen needs __________ additional electron(s) to complete its octet. A. 0 B. 1 C. 2 83
ANSWER : B Because the halogen elements have seven valence electrons, they only require one additional electron to form a full octet. 84
29. Generally alkali metals need to __________ to complete their octets A. do nothing (as they already have a full octet) B. gain 7 valence electrons C. lose 1 valence electron 85
answer : c Alkali metals have 1 valence electron on their outer shell. They are more stable when they have 8 valence electrons, so they want to lose that valence electron. They do this by bonding with other elements. When they lose their 1 valence electron, they have a full octet and are therefore stable. 86
30. Based on the electron configuration of sulfur, S, a sulfur atom will __________ valence electrons when bonding with lithium. A. gain 2 B. lose 6 C. gain 6 87
answer : a The electronic configuration of sulfur shows that it has six valence electrons and since the subshell p is incomplete it needs two electrons more to gain stability . So it forms a sulphide ion by gaining two electrons. 88