Chp 6 - Honors Chem

Flashcard 1:

Term: Mendeleev
Definition: Formulated the periodic law and arranged elements by increasing atomic mass, predicting the properties of undiscovered elements.

Flashcard 2:

Term: Moseley
Definition: Established the atomic number based on protons and arranged the periodic table by atomic number.

Flashcard 3:

Term: Periodicity
Definition: Recurring patterns in element properties as you move across periods and groups in the periodic table.

Flashcard 4:

Term: Electrostatic Force
Definition: The force of attraction between positively charged protons and negatively charged electrons, influenced by distance and shielding.

Flashcard 5:

Term: Periodic Law
Definition: Elements ordered by increasing atomic number show repeating patterns in their physical and chemical properties.

Flashcard 6:

Term: Valence Electrons
Definition: Electrons in the outermost energy level of an atom, crucial for bonding and reactivity.

Flashcard 7:

Term: Core/Kernel Electrons
Definition: Electrons in energy levels that are not the outermost level, contributing to the shielding effect.

Flashcard 8:

Term: Alkaline Earth Metals
Definition: Group 2 elements that are reactive, have low densities, melting points, and form basic solutions (pH > 7).

Flashcard 9:

Term: Transition Metals
Definition: Elements with valence electrons in two different shells, often forming colored compounds and used as catalysts.

Flashcard 10:

Term: Alkali Metals
Definition: Group 1 elements, highly reactive and electropositive, known for forming 1+1+ cations.

Flashcard 11:

Term: Metals
Definition: Elements that are ductile, malleable, lustrous, and good conductors of heat and electricity.

Flashcard 12:

Term: Nonmetals
Definition: Elements that are brittle, poor conductors, and often have high electronegativities.

Flashcard 13:

Term: Metalloids
Definition: Elements with properties intermediate between metals and nonmetals, useful as semiconductors.

Flashcard 14:

Term: Halogens
Definition: Group 17 elements that are highly reactive, electronegative, and typically toxic.

Flashcard 15:

Term: Noble Gases
Definition: Group 18 elements with full valence electron shells, chemically inert and nonreactive.

Flashcard 16:

Term: Atomic Radius Trends
Definition: Increases down a group and decreases across a period due to changes in nuclear charge and shielding.

Flashcard 17:

Term: Ionic Radius Trends
Definition: Increases down a group and decreases across a period, similar to atomic radius trends.

Flashcard 18:

Term: Electronegativity
Definition: A measure of an atom’s ability to attract electrons in a bond, increasing across periods and decreasing down groups.

Flashcard 19:

Term: Ionization Energy
Definition: The energy required to remove an electron from an atom, increases across a period and decreases down a group.

Flashcard 20:

Term: Cations
Definition: Positively charged ions formed by the loss of electrons.

Flashcard 21:

Term: Anions
Definition: Negatively charged ions formed by the gain of electrons.

Flashcard 22:

Term: Nuclear Charge
Definition: The total charge in the nucleus due to protons, influencing the force of attraction on electrons.

Flashcard 23:

Term: Shielding Effect
Definition: Core electrons reduce the attractive force between the nucleus and valence electrons.

Flashcard 24:

Term: First Ionization Energy
Definition: The energy required to remove the first electron from an atom, forming a cation.

Flashcard 25:

Term: Second Ionization Energy
Definition: The energy required to remove a second electron, creating a new cation.

Flashcard 26:

Term: Covalent Bonds
Definition: A type of bond where electrons are shared between atoms; can be polar (uneven sharing) or nonpolar (even sharing).

Flashcard 27:

Term: Ionic Bonds
Definition: Bonds formed by the transfer of electrons between atoms, typically between metals and nonmetals.

Flashcard 28:

Term: Polar Bonds
Definition: Bonds with unequal sharing of electrons, leading to partial charges.

Flashcard 29:

Term: Nonpolar Bonds
Definition: Bonds with equal sharing of electrons, resulting in no charge separation.

Flashcard 30:

Term: Malleable
Definition: The ability of a material (usually metals) to be hammered into thin sheets without breaking.

Flashcard 31:

Term: Coulombic Forces
Definition: The force of attraction between positive and negative charges in an atom, affecting many atomic properties.