Periodic Table and Chemical Bonding Quiz

Chemistry Lesson on the Periodic Table and Chemical Bonding

• The atomic number at the top of the periodic table is the number of protons and electrons in an atom, and the mass number at the bottom is the sum of protons and neutrons.

• Isotopes are atoms of the same element with different atomic masses due to different numbers of neutrons.

• The mass number with a decimal point represents the weighted average of an element's isotopes.

• Carbon has two isotopes, Carbon-12 and Carbon-14, with the latter being radioactive and used in radiometric dating.

• The valence shell of an atom contains the outermost electrons, which participate in chemical reactions, and the octet rule states that atoms tend to gain or lose electrons to achieve a full valence shell of eight electrons.

• Chemical bonds include ionic, covalent, and metallic bonds, and are formed to achieve a full valence shell.

• In an ionic bond, one atom transfers an electron to another atom to achieve a full valence shell, resulting in positive and negative ions that attract each other due to opposite charges.

• Non-metals tend to gain electrons, while metals tend to lose electrons, and if a metal and a non-metal are combined, an ionic bond is formed.

• In a covalent bond, atoms share electrons in order to achieve a full valence shell.

• Noble gases are inert because their valence shells are already full.

• Metalloids are in between metals and non-metals, and their properties depend on the specific element.

• The crystal structure of an ionic compound, such as table salt, results from the precise arrangement of positive and negative ions to minimize electrostatic repulsion.Chemical Bonding: Ionic and Covalent Bonds

• When a metal bonds with a non-metal, the metal transfers electrons to the non-metal, forming an ionic bond.

• When two non-metals bond, they share electrons, forming a covalent bond.

• The number of covalent bonds an atom can form is determined by how many spaces it is away from the noble gases on the periodic table.

• Carbon can form four covalent bonds and commonly bonds with hydrogen to form methane (CH4).

• Nitrogen forms three covalent bonds and bonds to itself in the atmosphere to form a triple bond.

• Nitrogen is difficult to separate because it is held together tightly, and 80% of the air we breathe is nitrogen.

• Water is a polar molecule because the electrons are shared unequally between oxygen and hydrogen atoms.

• Metals only want to give away electrons, so when two metals bond, they simply give electrons to each other.

• The number of valence electrons in a column (or family) on the periodic table determines how atoms in that column will behave in a chemical reaction.

• As we move across a row (or period) on the periodic table, the properties of the elements change slightly.

• Lithium is very metallic, while the most non-metallic element is on the opposite side of the periodic table.

• When two metals bond, they do not form ions or molecules, but simply share electrons.

Chemistry Lesson on the Periodic Table and Chemical Bonding

• The atomic number at the top of the periodic table is the number of protons and electrons in an atom, and the mass number at the bottom is the sum of protons and neutrons.

• Isotopes are atoms of the same element with different atomic masses due to different numbers of neutrons.

• The mass number with a decimal point represents the weighted average of an element's isotopes.

• Carbon has two isotopes, Carbon-12 and Carbon-14, with the latter being radioactive and used in radiometric dating.

• The valence shell of an atom contains the outermost electrons, which participate in chemical reactions, and the octet rule states that atoms tend to gain or lose electrons to achieve a full valence shell of eight electrons.

• Chemical bonds include ionic, covalent, and metallic bonds, and are formed to achieve a full valence shell.

• In an ionic bond, one atom transfers an electron to another atom to achieve a full valence shell, resulting in positive and negative ions that attract each other due to opposite charges.

• Non-metals tend to gain electrons, while metals tend to lose electrons, and if a metal and a non-metal are combined, an ionic bond is formed.

• In a covalent bond, atoms share electrons in order to achieve a full valence shell.

• Noble gases are inert because their valence shells are already full.

• Metalloids are in between metals and non-metals, and their properties depend on the specific element.

• The crystal structure of an ionic compound, such as table salt, results from the precise arrangement of positive and negative ions to minimize electrostatic repulsion.Chemical Bonding: Ionic and Covalent Bonds

• When a metal bonds with a non-metal, the metal transfers electrons to the non-metal, forming an ionic bond.

• When two non-metals bond, they share electrons, forming a covalent bond.

• The number of covalent bonds an atom can form is determined by how many spaces it is away from the noble gases on the periodic table.

• Carbon can form four covalent bonds and commonly bonds with hydrogen to form methane (CH4).

• Nitrogen forms three covalent bonds and bonds to itself in the atmosphere to form a triple bond.

• Nitrogen is difficult to separate because it is held together tightly, and 80% of the air we breathe is nitrogen.

• Water is a polar molecule because the electrons are shared unequally between oxygen and hydrogen atoms.

• Metals only want to give away electrons, so when two metals bond, they simply give electrons to each other.

• The number of valence electrons in a column (or family) on the periodic table determines how atoms in that column will behave in a chemical reaction.

• As we move across a row (or period) on the periodic table, the properties of the elements change slightly.

• Lithium is very metallic, while the most non-metallic element is on the opposite side of the periodic table.

• When two metals bond, they do not form ions or molecules, but simply share electrons.

Introduction to Minerals and Mineral Groups

• Cleavage is how a mineral breaks, and a mineral can have more than one plane of cleavage.
• Halite has three directions of cleavage, while mica has perfect cleavage in one direction only.
• Minerals have different chemical properties, such as taste, malleability, magnetism, and reaction to hydrochloric acid.
• The two main categories of mineral groups are rock-forming minerals and non-rock-forming minerals.
• Silicates make up most of the rocks around us, and the crust of the Earth is mostly composed of silicates.
• The eight most common elements in rock-forming minerals are oxygen, silicon, aluminum, iron, calcium, sodium, potassium, and magnesium.
• Oxygen and silicon are the top two most commonly occurring elements in rock-forming minerals.
• The basic building block of silicate minerals is the silicon-oxygen tetrahedron, which can attach to other tetrahedra or metal atoms to form silicates.
• Silicates can be classified into several subgroups based on their chemical composition and crystal structure.
• Non-silicate minerals include sulfates, carbonates, oxides, halides, and native elements.
• Minerals play important roles in various applications, such as construction, electronics, medicine, and energy production.
• Understanding minerals and mineral groups is crucial for geologists, mineralogists, and other scientists to study Earth's history, processes, and resources.

Introduction to Minerals and Mineral Resources

• Silicate minerals are composed of silicon-oxygen tetrahedrons that bond together in various structures.
• Olivine is an example of isolated tetrahedrons with metal atoms at each corner, making up the mineral olivine.
• Peridot is a precious variety of olivine.
• Single chains of tetrahedrons make up a general category of minerals called pyroxene, and a specific example is agite.
• Amphibole is made up of double chains of tetrahedrons, while micas are composed of three-dimensional sheets.
• Quartz has a very orderly structure and is one of the most common minerals on the earth's surface.
• Light-colored silicates are less dense and primarily composed of feldspar, including potassium and plagioclase feldspar.
• Dark-colored silicates are primarily composed of olivine, pyroxene, amphibole, and micas.
• The remaining mineral groups include carbonates, halides, oxides, sulfides, sulfates, and native elements.
• Mineral resources can be renewable or non-renewable, with ore deposits being concentrations of minerals that can be mined for profit.
• Aluminum is a non-renewable resource that must be recycled due to its limited availability.
• A massive pit mine, such as the one shown, is an example of mining for mineral resources.