Ionic Compounds and Their Properties

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Questions and Answers

What happens to electrons during the formation of ionic bonds?

Electrons are shared between metal and nonmetal.

Electrons are gained by both metal and nonmetal.

Electrons are transferred from the metal to the nonmetal. (correct)

Electrons are lost by both metal and nonmetal.

Which of the following ions is classified as a cation?

S2-

O2-

Na+ (correct)

Cl-

Which type of compound follows a different naming rule compared to ionic compounds?

Binary molecular compounds

Ionic compounds

Acids (correct)

Metallic compounds

What does the term 'empirical formula' refer to in the context of ionic compounds?

The formula that represents the simplest ratio of ions. Signup and view all the answers

Which of the following is NOT a common cation?

Cl- Signup and view all the answers

Which model of the atom proposed by J.J. Thomson featured a positive sphere with negative electrons embedded in it?

Plum pudding model Signup and view all the answers

What was the key experiment that led to the discovery of the nucleus?

Shooting alpha particles at gold foil Signup and view all the answers

What did Rutherford postulate about the structure of the atom after his experiments?

Atoms contain a small, dense positive center with electrons surrounding it. Signup and view all the answers

Which of the following statements is true about protons and neutrons?

Both protons and neutrons have approximately the same mass. Signup and view all the answers

What is stated in Dalton’s atomic theory regarding the transformation of atoms?

Atoms of an element remain unchanged in chemical reactions. Signup and view all the answers

What is the atomic number of an element derived from?

The number of protons in the nucleus. Signup and view all the answers

What charge do electrons carry?

Negative (−1) Signup and view all the answers

Which discovery first led to the understanding that the atom is made of smaller particles?

Thomson's discovery of cathode rays Signup and view all the answers

Which of the following statements accurately describes neutrons?

Neutrons are neutral particles located in the nucleus. Signup and view all the answers

What was the charge of the electron determined by Millikan?

1.602 x 10^-19 C Signup and view all the answers

Which type of radiation is positively charged according to Rutherford's findings?

α particles Signup and view all the answers

How is the mass of an electron generally treated in atomic mass calculations?

It is not included as its mass is negligible. Signup and view all the answers

How did the discovery of radioactivity impact the understanding of atoms?

It showed that atoms are composed of smaller particles and possess energy. Signup and view all the answers

What can be concluded about the compounds formed from different elements?

They always have the same relative number and kind of atoms. Signup and view all the answers

What measurement allowed for the calculation of the charge/mass ratio of the electron?

Thomson's observations of cathode rays Signup and view all the answers

Which of the following was not one of the types of radiation discovered by Rutherford?

δ particles Signup and view all the answers

What is the formula for the acetate ion?

CH3COO⁻ Signup and view all the answers

Which of the following ions has a charge of 1-?

Hydroxide ion Signup and view all the answers

Which ion is represented by the formula ClO4⁻?

Perchlorate ion Signup and view all the answers

What is the charge of the bromide ion?

1- Signup and view all the answers

Which of the following anions contains nitrogen?

Nitrate ion Signup and view all the answers

Which ion is incorrectly paired with its formula?

Bromate ion - BrO3⁻ Signup and view all the answers

What is the correct name for the ion with the formula OH⁻?

Hydroxide ion Signup and view all the answers

Which of the following anions has the formula CN⁻?

Cyanide ion Signup and view all the answers

Which ion is known as the cupric ion?

Cu2+ Signup and view all the answers

What is the common charge of the iron(II) ion?

2+ Signup and view all the answers

Which of the following ions carries a +2 charge?

Ca2+ Signup and view all the answers

Which ion is referred to as the manganous ion?

Mn2+ Signup and view all the answers

Identify the name of the ion with the formula Hg2+.

Mercuric ion Signup and view all the answers

What is the chemical formula for the zinc ion?

Zn2+ Signup and view all the answers

Which of the following ions is known as the plumbous ion?

Pb2+ Signup and view all the answers

Which ion corresponds to the formula Ag+?

Silver ion Signup and view all the answers

What is the name of the ion with the formula Ni2+?

Nickelous ion Signup and view all the answers

Which of the following describes the charge of the cadmium ion?

2+ Signup and view all the answers

What is the name of the polyatomic cation NH4+?

Ammonium Signup and view all the answers

Which oxygen-containing ion is correctly paired with its name?

ClO3− : Chlorate Signup and view all the answers

How is the ion ClO4− named?

Perchlorate Signup and view all the answers

Which of the following correctly illustrates the nomenclature of an inorganic acid?

HBr : Hydrobromic acid Signup and view all the answers

Which of these pairs correctly identifies the charge of the specific oxoanions?

PO4 3− : Phosphate Signup and view all the answers

What is the proper way to name an anion ending with -ite?

Change to -ous acid Signup and view all the answers

Which prefix is used to indicate the presence of two atoms in binary molecular compounds?

Di- Signup and view all the answers

If an anion ends in -ate, how is the corresponding acid named?

Change the ending to -ic acid Signup and view all the answers

Study Notes

Chapter 2: Atoms, Molecules, and Ions

This chapter introduces atomic theory and subatomic particles.
Early Greek philosophers proposed the concept of the atom, believing it to be the smallest indivisible unit.
John Dalton's atomic theory, developed in the early 1800s, organized the earlier discoveries into a more structured model.
Dalton's theory was based on several laws:
- Law of constant composition: compounds always contain the same elements in the same proportions. Examples include H₂O, CO, and CO₂. This law was discovered by Joseph Proust.
- Law of conservation of mass: the total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place. This was discovered by Antoine Lavoisier.
- Law of multiple proportions: if two elements form more than one compound, the masses of one element that combine with a given mass of the other are in the ratio of small whole numbers. This was discovered by John Dalton. Example: CO vs. CO₂.

2.1 Atomic Theory of Matter

Greek philosophers like Democritus envisioned "atomos" (uncuttable) as fundamental particles making up all matter.
Experiments in the 18th and 19th centuries led to Dalton's organized model of atoms.

Postulates of Dalton's Atomic Theory

Each element is made up of extremely small particles called atoms.
All atoms of a given element are identical in mass and other properties but differ from atoms of other elements.
Atoms of one element cannot be changed into atoms of another element by chemical reactions.
Atoms of different elements combine in simple whole-number ratios to form chemical compounds.

2.2 Discovery of Subatomic Particles

Dalton's model viewed atoms as indivisible. But further discoveries revealed subatomic particles.
Electrons, discovered by J.J. Thomson in 1897, are negatively charged particles found in atoms.
Radioactivity, discovered by Henri Becquerel, demonstrates the atom's internal complexity and energy content.
Marie and Pierre Curie also studied radioactivity.
The nucleus, a tiny, dense, positively charged central core of the atom, and protons (positively charged) and neutrons (neutral) were discovered by Ernest Rutherford.

2.3 Modern View of Atomic Structure

Rutherford's gold foil experiment proved the existence of a dense, positively charged nucleus within the atom.
Most of the atom is empty space.
Atoms have a size of 1-5 Å (or 100-500 pm).
Atoms are made up of protons, neutrons, and electrons.

Subatomic Particles

Protons (+1), electrons (-1) have charges, while neutrons are neutral.
Protons and neutrons are approximately the same mass; electrons have much less mass.

Atomic Number

The atomic number identifies an element. It represents the number of protons within an atom's nucleus.
The number of protons equals the number of electrons in a neutral atom.

Atoms of an Element

Elements are represented by one or two-letter symbols (e.g., C for carbon).
Atomic number (number of protons) is written as a subscript before the symbol.
Mass number (protons + neutrons) is written as a superscript before the symbol.
Isotopes: atoms of the same element with different numbers of neutrons but the same number of protons. Example: ¹²C, ¹³C, ¹⁴C.

2.4 Atomic Mass Unit (amu)

Atoms have extremely small masses, and a scale using atomic mass units (amu) is used.
The atomic mass unit is relative to the mass of carbon-12 (¹²C), which is assigned a mass of exactly 12 amu. One amu is equal to 1.66054 × 10⁻²⁴ g

Atomic Weight

Since the isotopes ratios naturally exist, atomic weight is the average mass of an atom based on relative isotopes abundance.
It is determined by averaging the mass of an element's various isotopes with their relative abundance in nature.

Atomic Weight Measurement

Mass spectrometry is used to measure atomic and molecular weights, and the abundance of isotopes. Isotopes have similar chemical properties, but different masses.

2.5 Periodic Table

The periodic table organizes elements by atomic number (number of protons) and similar properties.
Elements are arranged in periods (rows) and groups (columns).
Elements in the same group have similar chemical properties, and have a repeating pattern of chemical behavior.

Reading the Periodic Table

Atomic number is listed above the element symbol.
Atomic weight is listed below the element symbol.

Organization of the Periodic Table

Rows are called periods, and columns are called groups.
Elements in the same group share similar physical and chemical properties, due to their similar electron configurations.

Periodicity - Rows

Elements in a row exhibit repeating properties and reactivities.

Groups - Columns

Groupings have named groups like Alkali metals, Alkaline earth metals, Chalcogens, Halogens, and Noble gases, these groups have related chemical properties.

2.6 Molecules and Molecular Compounds

A chemical formula uses subscripts to represent the number of each kind of atom in a molecule.
Molecular Compounds are made up of molecules almost always consisting of nonmetals.
Diatomic molecules occur naturally as molecules with two atoms. Examples include H₂, N₂, O₂, F₂, Cl₂, Br₂, and I₂

Types of Formulas

An empirical formula gives the lowest whole number ratio of atoms.
A molecular formula shows the exact number of atoms.

Picturing Molecules

Structural formulas (2D) display the order of attachment, not their shape.
Perspective drawings, ball-and-stick models, and space-filling models represent three-dimensional shape.

2.7 Ions and Ionic Compounds

Ions are formed when atoms gain or lose electrons.
Cations are positively charged ions (formed by metals).
Anions are negatively charged ions (formed by nonmetals except noble gases).
Ionic compounds generally form between metals and nonmetals. Transfer of electrons results in oppositely charged ions that attract each other.

Ionic Compounds

Ionic compounds are formed from charged particles called ions.
Oppositely charged ions attract, forming an ionic lattice structure.
Only empirical formulas are used to represent ionic compounds.

2.8 Naming Inorganic Compounds

Chemical nomenclature is the system of naming compounds.
Names of ions (cations and anions) are essential to memorize.
Rules exist for naming ionic compounds, acids, and binary molecular compounds.

Common Cations

Table 2.4 List of common cations with their charges and names including groups 1-A and 2-A elements. The transition metals are also included.

Common Anions

Table 2.5 List of common anions with their charges and names. The anions included in this table are monatomic anions like chloride or bromide. Polyatomic anions are also listed like perchlorate or phosphate.

Polyatomic Ions

Some groups of atoms act as ions and are called Polyatomic ions.

Writing Inorganic Formulas

The charges of the ions will determine the ratio of one element to another, the subscript for each element.

Naming Inorganic Compounds

Cations are named first, followed by anions.
Transition metals (having more than one ionic charge) require Roman numerals in parentheses.
Polyatomic ions have specific names. The rule for nonmetals such as chlorine is to change the ending to ide in the anion name.

Patterns in Oxyanion Nomenclature

Oxyanions (polyatomic anions containing oxygen) follow naming patterns based on the number of oxygen atoms.
The ion with fewer oxygen atoms ends in -ite. The ion with more oxygen atoms ends in -ate. These are also referred to as oxyanions.

Inorganic Acid Nomenclature

Acids with -ide ending of the anion name is changed to -ic acid with the prefix hydro- put before the name.
Acids with -ite ending of the anion name is changed to -ous acid.
Acids with -ate ending of the anion name is changed to -ic acid.

Nomenclature of Binary Molecular Compounds

The element farther to the left on the periodic table or lower in the same group is usually named first.
Prefixes are used to denote the numbers of atoms of each element. Examples are mono, di, tri....

2.9 Some Simple Organic Compounds

Organic chemistry is the study of carbon compounds and its branches for nomenclature.
Hydrocarbons (compounds with C and H) are alkanes.
The names follow prefixes based on the number of carbon atoms. (Example meth-, eth-, prop-...) followed by the suffix -ane in the name.

Nomenclature of Alcohols

Alcohols are hydrocarbons with -OH groups.
Their names are derived from the alkane by adding the suffix -ol to it.

Nomenclature Isomers: Alcohols

Isomers are compounds that have the same chemical formula but different structures.
Isomers are formed when the atoms are arranged differently but with the same molecular formula.

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Description

This quiz explores key concepts related to ionic bonding, including the behavior of electrons, ion classification, and empirical formulas. Test your understanding of the naming conventions related to ionic compounds and identify common cations. Perfect for students studying chemistry.