CR Chem Module 3 Lesson 2

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Questions and Answers

What property of metals is primarily responsible for their shiny appearance?

High boiling point

Electrical conductivity

Metallic luster (correct)

Malleability

Which of the following metals is known for its high electrical conductivity and is commonly used in wiring?

Tin

Lead

Copper (correct)

Iron

What characteristic allows metals to be shaped into thin sheets without breaking?

Malleability (correct)

Solubility

Ductility

Brittleness

What is the reason for the high melting and boiling points of metals?

Strong forces between metal cations and delocalized electrons Signup and view all the answers

In which part of the periodic table are metals typically located?

In the center and left side Signup and view all the answers

What typically happens when metals react with acids?

They produce hydrogen gas and a salt. Signup and view all the answers

Which of the following is a common property of metals?

Ability to conduct heat and electricity Signup and view all the answers

Which of the following properties is NOT characteristic of nonmetals?

Highly malleable and ductile. Signup and view all the answers

What property makes metals suitable for being drawn into wires?

Ductility Signup and view all the answers

In terms of reactivity, how do metals behave in the periodic table?

Reactivity increases as you move down a group. Signup and view all the answers

Which metal has one of the highest melting points, at 3422°C?

Tungsten Signup and view all the answers

What allows free electrons in metals to carry energy and electrical charge?

Free movement Signup and view all the answers

Which statement about nonmetals and their oxides is true?

Nonmetal oxides are usually acidic. Signup and view all the answers

Which of the following statements is NOT true about metals?

They usually have low melting points. Signup and view all the answers

What is true about the ionization energy of metals compared to nonmetals?

Metals have lower ionization energies than nonmetals. Signup and view all the answers

Why do nonmetals exhibit poor conductivity?

They have tightly bound electrons. Signup and view all the answers

Which of the following metals is known for its high density?

Lead Signup and view all the answers

What is the typical characteristic of metals in terms of electronegativity?

They generally have low electronegativity. Signup and view all the answers

What happens when sodium reacts to form a cation?

It loses one electron to form Na⁺. Signup and view all the answers

Which nonmetal is commonly used in water treatment processes?

Chlorine Signup and view all the answers

Study Notes

Metals

Metals occupy the left and center regions of the periodic table.
Characterized by shiny appearance known as metallic luster, due to free-moving electrons reflecting light.
Excellent conductors of heat and electricity, with copper and aluminum being prime examples.
Malleable and ductile; can be hammered into sheets or drawn into wires while maintaining structure.
High melting and boiling points, attributed to strong attractions between metal cations and delocalized electrons; tungsten has a melting point of 3422°C.
Generally high density; lead has a density of 11.34 g/cm³.
React with oxygen to form oxides; for example, iron and oxygen create iron oxide (rust).
React with acids to yield hydrogen gas and salts; zinc and hydrochloric acid produce zinc chloride and hydrogen.
Tend to lose electrons forming positively charged ions (cations), exemplified by sodium forming Na⁺.

Nonmetals

Found on the right side of the periodic table; properties are often the opposite of metals.
Lack metallic luster; most appear dull and do not reflect light.
Poor conductors of heat and electricity due to absence of free-moving electrons; sulfur and phosphorus exemplify this.
Typically brittle when solid, breaking rather than deforming; sulfur crystals are a common example.
Lower melting and boiling points compared to metals; graphite carbon melts at 3652°C, iodine at 113.7°C.
Generally lower densities; gases like hydrogen and helium have very low densities.
React with oxygen to form acidic oxides, such as carbon yielding carbon dioxide (CO₂).
Can react with bases to form salts and water, demonstrated by sulfur dioxide with sodium hydroxide.
Tend to gain electrons to form negatively charged ions (anions); chlorine forms Cl⁻.

Periodic Trends

Metals typically have low electronegativity, with levels increasing left to right and decreasing down a group.
Have low ionization energies which increase across periods and decrease down groups, facilitating cation formation.
Reactivity in metals generally increases down a group; alkali metals like potassium are highly reactive.
Nonmetals possess high electronegativity values, attracting electrons strongly; this trend mirrors that of metals.
Nonmetals have high ionization energies, resisting electron loss; this also follows the periodic trend.
Reactivity in nonmetals generally decreases down a group; for instance, halogens are more reactive than noble gases.

Practical Applications

Metals are crucial in construction (steel, aluminum), electronics (gold, silver, copper), and the automotive industry (iron, steel).
Nonmetals play key roles in water treatment (chlorine for disinfection), medicine (iodine, fluorine in antiseptics), and agriculture (nitrogen and phosphorus in fertilizers).
Understanding properties of these elements aids predictions in chemical interactions and applications in various sectors.

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Description

Explore the fundamental properties and behaviors of metals and nonmetals in this quiz. Gain insights into how these two categories of elements interact and form compounds. This overview emphasizes their physical and chemical properties, which are crucial in understanding chemistry.