Periodic Table Quiz & Flashcards

Elements are arranged by increasing atomic number, not mass or reactivity.

Fluorine is the most electronegative due to its small size and high nuclear charge.

Noble gases have full valence shells, making them unreactive; they are non-metals.

Atomic radius increases because additional electron shells are added.

Group 1 elements, the alkali metals, are the most reactive metals.

Transition metals have multiple oxidation states, unlike most other metals.

Ionization energy increases as nuclear charge increases within a period.

Alkali metals have one valence electron, making them very reactive as they easily lose it.

Smaller atomic radii result in higher electronegativity due to stronger nuclear attraction.

Periods are horizontal rows; groups are vertical columns.

Halogens are known as 'salt-formers' because they easily form salts with metals.

Elements in the same group have similar reactivity due to the same number of valence electrons.

Fluorine is the only halogen in the second period.

Metalloids exhibit properties of both metals and non-metals, found along the zig-zag line.

Melting points generally increase to a peak and then decrease across a period.

Lanthanides are known for their rare earth properties, often used in specialized alloys.

Electron affinity increases across a period as the nuclear charge increases.

Actinides are known for their radioactivity, especially those beyond uranium.

Calcium is a typical alkaline earth metal with properties distinct from alkali metals.

Valence electrons are involved in the formation of chemical bonds, determining reactivity.

Reactivity decreases due to increased atomic size and weaker attraction for electrons.

Carbon-12 is used as the standard for atomic masses, defining the atomic mass unit.

Noble gases are inert and do not react, making them safe for use in lighting.

Transition metals are commonly used as catalysts due to their flexible oxidation states.

Silicon is a metalloid with properties between metals and non-metals.

Atomic size decreases due to increased nuclear charge pulling electrons closer.

Periodicity arises from repeating patterns in electron configurations across periods.

Sodium tends to lose an electron to form a cation, unlike non-metals like chlorine.

Calcium is an alkaline earth metal, not a transition metal.

Ionization energy decreases down a group due to increased atomic size.

Hydrogen's unique properties do not fit a single group, so it is placed separately.

Electronegativity increases across a period due to increasing nuclear charge.

Neon is a noble gas, known for its lack of chemical reactivity.

Alkaline earth metals have two valence electrons, making them reactive but less so than alkali metals.

Electronegativity decreases down a group due to increased atomic size.

Cesium has the largest atomic radius as it is the furthest down Group 1.

Gold is located in Period 6 of the periodic table.

Alkali metals commonly have a +1 oxidation state due to losing one electron.

Density generally increases toward the middle of a period and decreases thereafter.

Most actinides are radioactive, especially those beyond uranium.

Phosphorus is part of Group 15, the nitrogen group, known for forming compounds with varied oxidation states.

Elements form compounds to achieve a stable electronic configuration with a full valence shell.

Neon has the highest first ionization energy due to its full valence shell and high effective nuclear charge.

Elements in the same period share the same number of electron shells.

Iodine is a halogen, known for being reactive and forming salts.

Oxygen commonly has an oxidation state of -2, forming oxides with most elements.

Electronegativity decreases down a group as atomic size increases.

Argon is a noble gas, characterized by its inertness due to a full valence shell.