Chemistry Chapter: Atomic Notation and Ions

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Questions and Answers

Which group on the periodic table contains elements that are the least reactive due to their filled outer shells?

Group IIA (Alkaline Earth Metals)

Group VIIIA (Noble Gases) (correct)

Group VIIA (Halogens)

Group 1A (Alkali Metals)

What is the primary factor that influences the trend in atomic radius across a period from left to right?

The number of valence electrons

The number of electron shells

The number of neutrons in the nucleus

The number of protons in the nucleus (correct)

Which of the following statements is TRUE about the reactivity of metals in the periodic table?

Reactivity increases from right to left and decreases going down the periodic table.

Reactivity increases from left to right and decreases going down the periodic table.

Reactivity increases from left to right and increases going down the periodic table.

Reactivity increases from right to left and increases going down the periodic table. (correct)

What is the difference between average atomic mass and relative atomic mass?

Average atomic mass is calculated for a specific sample, while relative atomic mass is an average of all isotopes in a standard environment. Signup and view all the answers

What effect does an increase in the number of electron shells (orbits) have on the atomic radius?

It increases the atomic radius. Signup and view all the answers

Which of the following best describes the trend of non-metal reactivity in the periodic table?

Increases from left to right and decreases going down the periodic table. Signup and view all the answers

Why are halogens (Group VIIA) highly reactive?

They lack one electron to fill their outer shell, making them eager to gain an electron. Signup and view all the answers

Which of the following factors influences the effective nuclear charge experienced by the outermost electrons?

The number of protons Signup and view all the answers

What is the primary reason that cations are always smaller than their parent atoms?

Cations lose electrons, reducing electron-electron repulsion. Signup and view all the answers

Which of the following statements about ionization energy is true?

Ionization energy increases down a group due to increased electron shielding. Signup and view all the answers

What trend is observed in electron affinity as you move from left to right across a period?

Electron affinity increases for all elements. Signup and view all the answers

Why is fluorine considered to have the highest electronegativity?

Fluorine's effective nuclear charge is higher, attracting electrons more effectively. Signup and view all the answers

How does the size of an atom relate to its ionization energy?

Larger atoms generally have lower ionization energy due to increased distance from nucleus. Signup and view all the answers

Which of the following statements best defines electronegativity?

Electronegativity is the ability of an atom to attract bonding electrons to itself. Signup and view all the answers

What is the effect of effective nuclear charge on electronegativity?

Higher effective nuclear charge results in stronger attraction for bonding electrons. Signup and view all the answers

What is the significance of the electronegativity difference (∆EN) in bond formation?

It predicts the ionic or covalent nature of a bond between atoms. Signup and view all the answers

Which of the following statements accurately describes the octet rule?

Atoms strive to gain or lose electrons to achieve a stable configuration with eight valence electrons. Signup and view all the answers

What is the difference between an atom and an ion?

An atom is neutral, while an ion has a charge. Signup and view all the answers

Identify the correct name for the ion formed by the element bromine (Br).

Bromide ion Signup and view all the answers

Which of the following statements correctly describes isotopes?

Isotopes are atoms of the same element with different numbers of neutrons. Signup and view all the answers

Which type of radiation is a high-energy electromagnetic wave?

Gamma ray Signup and view all the answers

Using the mnemonic 'NICK the CAMEL ate a CLAM for SUPPER in PHOENIX,' what is the formula for the 'ate' form of the polyatomic ion containing phosphorus (P)?

PO4^-3 Signup and view all the answers

Which of the following represents the 'ite' form of the polyatomic ion containing sulfur (S)?

SO3^-2 Signup and view all the answers

What is the primary difference between a radioisotope and a stable isotope?

A radioisotope undergoes spontaneous decay, while a stable isotope does not. Signup and view all the answers

Study Notes

Standard Atomic Notation

Mass Number (A) = number of protons (Z) + number of neutrons (N)
Symbol (X) = chemical symbol for the element
Atomic Number (Z) = number of protons in the atom's nucleus
Atomic Mass Unit (u) = 1/12 the mass of one carbon-12 atom (1.660 540 2 x 10^-27 kg)

Ions and Octet Rule

Elements with a full valence shell (octet) are stable.
Atoms that don't have a full octet tend to combine with other atoms to achieve a stable octet by sharing, losing, or gaining electrons.
Ions are formed when atoms lose or gain electrons, creating a positive or negative charge.
Positive ions (cations) are formed when metals lose electrons.
Negative ions (anions) are formed when nonmetals gain electrons.

Multivalent Elements

Some elements can form more than one type of stable ion.
Transition metals are often multivalent.
Different charges are often represented using Roman numerals (e.g., copper(I) and copper(II)).

Polyatomic Ions

Ions containing more than one atom that act as a single unit.
Students should memorize common polyatomic ions.
Mnemonic device provided for memorization (NICK the CAMEL ate a CLAM for SUPPER in PHOENIX).

Ions in the Human Body

About 99% of the human body is composed of oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus.
Other elements like sulfur, chlorine, sodium, magnesium, iodine, and iron are present in smaller amounts, playing key roles.
Many elements are dissolved in water within the body.

Isotopes, Radioisotopes, and Atomic Mass

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons.
Isotopic abundance is the percentage of a particular isotope in a sample.
Atomic mass is the average mass of all isotopes of an element in a naturally occurring sample.

Average Atomic Mass

The average mass of an element considering the prevalence of the isotopes naturally.
Relative atomic mass is the average weight of all isotopes in a normal environment on the Earth's crust.

Periodic Table and Periodic Law

Elements in the same vertical column (group) have similar characteristics.
Groups IA (group 1) alkali metals, IIA (Group 2) alkaline earth metals, VIIA (Group 17) halogens, and VIIIA (Group 18) noble gases are notable periodic table groups.
Transition metals are in groups 3-12.
Inner transition metals are lanthanides (57 -70) and actinides (89-102).

Electron Configuration and Trends

Electron shielding influences the attractive force between electrons and the nucleus.
More orbits (larger atoms) = less effective nuclear charge.
More protons (smaller atoms) = stronger effective nuclear charge.
Atomic radius increases going down a group and decreases going across a period.
Metal reactivity increases going down a group and decreasing across a period.
Nonmetal reactivity increases going up a group and increasing across a period.

Ionic Radius

Cations are always smaller than the corresponding atom because the loss in electrons reduces the electron-electron repulsion.
Anions are always larger because the gain of electrons leads to increased repulsion among electrons.

Ionization Energy

Energy required to remove an electron from an atom or ion.
First ionization energy (IE₁), second ionization energy (IE₂), etc.
Removal becomes increasingly difficult for successive electrons.
Ionization energy increases going across a period and decreases going down a group.

Electron Affinity

Energy change that occurs when an electron is added to a neutral atom.
Higher electron affinity means more energy is released when an electron is added.
Electron Affinity increases across a period and decreases down a group.

Electronegativity

Ability of an atom to attract electrons in a covalent bond.
Electronegativity increases across a period.
Electronegativity decreases down a group.

Polar Bonds and Molecules

Differences in electronegativity result in bonds with unequal sharing of electrons (polar covalent).
Polar molecules have distinct positive and negative ends due to asymmetrical charge distribution.
Non-polar molecules have equal sharing of electrons (nonpolar covalent) and symmetrical distribution of charge.

Intermolecular Forces

Forces of attraction between molecules.
London dispersion forces (temporary dipoles), dipole-dipole forces (permanent dipoles).
Hydrogen bonds (strong dipole-dipole forces when hydrogen is bonded to nitrogen, oxygen, or fluorine).

Chemical Formulas

Binary molecular compounds - molecular formulas, and prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca).
Binary ionic compounds - include metal and nonmetal, find charge of each using periodic table and crossover to find subscript.

Nomenclature of Acids

Naming Binary acids (hydro ____ acid).
Naming Oxyacids (____ ic acid or ____ ous acid).
Naming Oxyacids with polyatomic ions (use naming rules for polyatomic ions).

Hydrates

Ionic compounds that contain bound water molecules in their crystal structure.
Hydrates are often referred to as the 'water of hydration'.

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Description

Dive into the fundamentals of atomic notation, ions, and the octet rule in this quiz. Explore mass numbers, atomic symbols, and the behavior of multivalent elements. Perfect for students looking to solidify their understanding of chemical principles.