Periodic Table & Chemical Elements Quiz

Alkaline earth metals have two valence electrons.

Halogens gain one electron to fill their outer electron shells.

Noble gases are unreactive due to having completely filled electron shells.

<p>Atomic radii increase as you move from top to bottom in the periodic table.</p> Signup and view all the answers

<p>Elements in Group 17 are called halogens, and they have seven valence electrons.</p> Signup and view all the answers

<p>Atomic radius is defined as one-half the distance between the centers of two atoms in a homonuclear diatomic molecule.</p> Signup and view all the answers

<p>Ionization energy generally increases as you move from left to right across the periodic table.</p> Signup and view all the answers

<p>The filled electron shells in noble gases contribute to their chemical inertness.</p> Signup and view all the answers

<p>It states that properties of elements are periodic functions of their atomic mass.</p> Signup and view all the answers

<p>He left gaps in his table to represent the unknown elements and predicted their properties based on the properties of surrounding elements.</p> Signup and view all the answers

<p>The Modern Periodic Law states that properties repeat based on increasing atomic number, rather than atomic mass.</p> Signup and view all the answers

<p>Noble gases were later discovered and could be placed in a separate group without disrupting the existing order of Mendeleev's table.</p> Signup and view all the answers

<p>The Alkali Metals include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr).</p> Signup and view all the answers

<p>They are arranged in a grid of 18 columns (groups) and 7 rows (periods), with a double row of elements below the main table.</p> Signup and view all the answers

<p>Both Barium and Sodium can form ions, illustrating their chemical reactivity based on their position in the periodic table.</p> Signup and view all the answers

<p>Their discovery confirmed the existence of properties that could be categorized without altering the arrangement of existing elements.</p> Signup and view all the answers

<p>Atomic size decreases from left to right due to increasing nuclear charge without a corresponding increase in electron shielding, pulling valence electrons closer to the nucleus.</p> Signup and view all the answers

<p>A cation is smaller than its neutral atom because losing an electron reduces electron-electron repulsion and eliminates the outermost shell.</p> Signup and view all the answers

<p>Mg is larger than Mg++ because upon losing two electrons to form Mg++, the increased effective nuclear charge attracts the remaining electrons more strongly, reducing the size.</p> Signup and view all the answers

<p>Anions are larger than their neutral atoms due to the addition of electrons, which increases electron-electron repulsion and pushes the electrons further apart.</p> Signup and view all the answers

<p>Ionization energy generally increases across a period as atomic size decreases, leading to stronger nuclear attraction making it harder to remove an electron.</p> Signup and view all the answers

<p>Coulombic law shows that atomic size is affected by the attraction between charged particles, represented by the formula: Fα q1q2/r².</p> Signup and view all the answers

<p>Ionic size of anions is larger than their neutral atoms due to an increase in negative charge and resulting electron-electron repulsion.</p> Signup and view all the answers

<p>Atomic size increases down a group because additional electron shells are added, which outweighs the effect of increased nuclear charge.</p> Signup and view all the answers

<p>The ionization energy increases as the size of the atom decreases because valence electrons are closer to the nucleus and harder to remove.</p> Signup and view all the answers

<p>Electron shielding reduces the effective nuclear charge felt by valence electrons, leading to a decrease in ionization energy from top to bottom in a group.</p> Signup and view all the answers

<p>Nitrogen has a higher ionization potential due to its half-filled p subshell, providing extra stability compared to carbon and oxygen.</p> Signup and view all the answers

<p>Electron affinity is the energy released when a neutral atom gains an electron; a more negative value indicates a higher tendency to attract electrons.</p> Signup and view all the answers

<p>Electron affinity generally becomes less negative as you move down a group due to increased atomic size and electron-electron repulsions.</p> Signup and view all the answers

<p>Electron affinity becomes more negative across a period because the atomic size decreases, enhancing the nucleus's attraction for added electrons.</p> Signup and view all the answers

<p>Electronegativity measures an atom's ability to attract electrons in a covalent bond and determines bond polarity.</p> Signup and view all the answers

<p>The octet rule drives the increase in electron affinity across a period as elements become more stable when achieving a full valence shell.</p> Signup and view all the answers

<p>Electronegativity increases across a period and decreases down a group.</p> Signup and view all the answers

<p>As atomic radius increases down a group, electronegativity decreases because the valence electrons are farther from the nucleus.</p> Signup and view all the answers

<p>Stronger bonds require more energy to break, leading to higher melting points for those elements.</p> Signup and view all the answers

<p>Metallic character decreases across a period and increases down a group.</p> Signup and view all the answers

<p>Non-metallic character is the tendency of an element to gain electrons and increases across a period but decreases down a group.</p> Signup and view all the answers

<p>Metalloids exhibit properties of both metals and non-metals; examples include Boron and Silicon.</p> Signup and view all the answers

<p>The energy required to gain electrons decreases as elements become more electronegative.</p> Signup and view all the answers

<p>Losing electrons becomes easier down a group due to increased atomic size, which means outer electrons are farther from the nucleus.</p> Signup and view all the answers