Metals and Non-Metals Lecture Notes

These flashcards cover key vocabulary and concepts discussed in the Metals and Non-Metals lecture.

Metals

Elements that are typically solid at room temperature (except for mercury), conductive of heat and electricity, malleable, ductile, and have high melting and boiling points.

Non-Metals

Elements that are often gaseous or brittle solids at room temperature, poor conductors of heat and electricity, and have low melting points.

Ionic Bonding

The electrostatic attraction between cations and anions, formed when electrons are transferred from a metal to a non-metal.

Electron-Sea Model

A theory that explains the properties of metals, in which metal cations are surrounded by a sea of delocalized electrons.

Specific Heat Capacity

The amount of energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius.

Valence Electrons

Electrons present in the outermost shell of an atom that can participate in forming bonds.

Octet Rule

Atoms tend to react to obtain a full outer shell of eight electrons.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Metalloids

Elements that have properties intermediate between metals and non-metals and are often used in semiconductors.

Conductivity

The ability of a material to conduct electricity or heat.

Ductility

The ability of a material to be drawn into wires.

Malleability

The ability of a material to be hammered or pressed into thin sheets.

Crystalline Structure

A solid material whose constituents, such as atoms, ions, or molecules, are arranged in a highly ordered structure.

States of Matter

The distinct forms that different phases of matter take on, commonly solid, liquid, and gas.

Electronegativity

The tendency of an atom to attract a bonding pair of electrons.

Polar Covalent Bond

A type of covalent bond in which electrons are not shared equally between atoms.

Non-Polar Covalent Bond

A type of covalent bond where electrons are shared equally between two identical nonmetals.

Naming Ionic Compounds

Compounds formed from metals and non-metals named using the metal name followed by the non-metal with the suffix '-ide'.

Transition Metals

Elements found in groups 3-12 of the periodic table, characterized by variable valence.

Halogens

Group 17 elements that typically have seven valence electrons.

Alkaline Earth Metals

Group 2 elements that typically have two valence electrons.

Alkali Metals

Group 1 elements that typically have one valence electron.

Noble Gases

Group 18 elements that are inert due to having full valence shells.

Ionization Energy

The energy required to remove an electron from an atom.

Atomic Mass

The mass of an atom, typically measured in atomic mass units (amu).

Group (Periodic Table)

Vertical column in the periodic table that contains elements with similar properties.

Period (Periodic Table)

Horizontal row in the periodic table in which elements have the same number of electron shells.

Calorimetry

The measurement of heat transfer in physical and chemical processes.

Electrostatic Attraction

The force of attraction between positively charged ions and negatively charged ions.

Metallic Bonding

Chemical bonding that occurs between metal atoms when they share a 'sea' of delocalized valence electrons.

Hydrogen

The lightest and most abundant chemical element, with one proton and one electron.

Lithium

A soft, silvery-white metal, and the lightest metal and element.

Beryllium

A chemical element which is a metal known for its high melting point and low density.

Boron

A metalloid that is essential for plant growth and occurs naturally in various compounds.

Carbon

A non-metal that is fundamental to life, making up the organic compounds.

Nitrogen

A non-metal that makes up about 78% of the Earth's atmosphere.

Oxygen

A vital non-metal element for respiration and combustion processes.

Fluorine

A highly reactive non-metal, the most electronegative element.

Neon

An inert noble gas used in neon signs, known for its bright colors when electrified.

Sodium

A soft, silvery-white, highly reactive metal, one of the alkali metals.

Magnesium

A shiny gray solid that has low density and is essential for biological functions.

Sulfur

A non-metal element that is essential for life and is predominantly found in proteins.

Silicon

A metalloid used extensively in semiconductors and electronic devices.

Phosphorus

A vital element in nucleic acids and ATP, essential for life.

Chlorine

A greenish-yellow gas that is a highly reactive non-metal, used in disinfectants.

Argon

An inert noble gas that is often used in light bulbs.

Copper

A ductile metal known for its electrical conductivity.

Zinc

A metallic element used for galvanization to protect against rust.

Iron

A strong metal, essential for biological processes, found in hemoglobin.

Lead

A dense metal that is often used in batteries and radiation shielding.

Gold

A highly valued metal known for its malleability and resistance to corrosion.

Sodium Chloride

An ionic compound also known as table salt, formed from sodium and chlorine.

Water (H2O)

A covalent compound essential for life, made from two hydrogen atoms and one oxygen atom.

Covalent Bonds

Bonds formed by the sharing of electrons between atoms.

Density

The mass per unit volume of a substance.

Metalloid Characteristics

Metalloids possess properties of both metals and non-metals.

Frying Pan Construction

The choice of metal for frying pans is influenced by the specific heat capacity.

Heat Transfer

The movement of energy from a warmer object to a cooler object.