Chemistry Chapter 6 Quiz

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Questions and Answers

Which acid has the suffix –ous based on the anion that ends in –ite?

H2SO3 (correct)

H2SO4

HNO3

HClO4

What is the correct name for HCN?

Hydrosulfuric acid

Hydrochloric acid

Nitric acid

Hydrocyanic acid (correct)

Which of the following compounds is named correctly?

Sn(OH)4 - tin(II) hydroxide

CaCrO4 - calcium chromate (correct)

H2SO4 - sulfurous acid

TiO2 - titanium(IV) oxide

Which of the following is the correct name for HNO2?

Nitrous acid Signup and view all the answers

What is the naming rule for acids that contain an anion ending in –ate?

Add the suffix –ic to the root name. Signup and view all the answers

What did Thomson postulate about electrons?

They are negatively charged particles. Signup and view all the answers

What is the primary characteristic of the nucleus of an atom?

It is extremely dense and accounts for most of the atom's mass. Signup and view all the answers

How do isotopes of an element differ?

They have different numbers of neutrons. Signup and view all the answers

Which particle in an atom has no charge?

Neutron Signup and view all the answers

What best describes the arrangement of electrons in the atom?

They are found outside the nucleus at large distances. Signup and view all the answers

What does the charge of a proton equal?

Positive, equal in magnitude to an electron's. Signup and view all the answers

What did Rutherford contribute to atomic theory?

He proposed the planetary model with a nucleus. Signup and view all the answers

Which of the following statements about isotopes is true?

They have the same number of electrons. Signup and view all the answers

What is the charge of Alkali Metals in Group 1A?

1+ Signup and view all the answers

Which of the following is a correct example of a Binary Ionic Compound (Type I)?

MgBr2 Signup and view all the answers

Which naming convention is applied to monatomic anions?

Use the root of the element name and add –ide Signup and view all the answers

Which of the following statements is true about Binary Ionic Compounds (Type II)?

The charge on the metal ion must be specified. Signup and view all the answers

Which of the following is an example of a Binary Ionic Compound (Type II)?

Iron(II) sulfide Signup and view all the answers

What is the characteristic of Noble Gases in Group 8A?

They have a neutral charge of 0 Signup and view all the answers

What does the mass number of an isotope represent?

The total number of protons and neutrons Signup and view all the answers

What must be memorized for naming compounds that contain them?

Polyatomic Ions Signup and view all the answers

What distinguishes Type I Binary Ionic Compounds from Type II?

Type I has a fixed charge cation Signup and view all the answers

Which of the following statements about ionic bonds is true?

They result from attraction between oppositely charged ions Signup and view all the answers

If an isotope has 54 electrons and 78 neutrons, what is its mass number?

133 Signup and view all the answers

Which of the following compounds contains a polyatomic ion?

NaOH Signup and view all the answers

Who is considered the first chemist for performing quantitative experiments?

Robert Boyle Signup and view all the answers

Which of the following correctly describes isotopes?

Isotopes have different mass numbers due to different numbers of neutrons Signup and view all the answers

How is the second element named in a binary covalent compound?

Like an anion Signup and view all the answers

What distinguishes cations from anions?

Cations have a positive charge, while anions have a negative charge Signup and view all the answers

What prefix is never used for the first element in a binary covalent compound?

mono- Signup and view all the answers

Which law states that mass is neither created nor destroyed in a chemical reaction?

Law of Conservation of Mass Signup and view all the answers

What is the significance of groups or families in the periodic table?

They include elements that exhibit similar chemical properties Signup and view all the answers

Which of the following best summarizes Dalton's Atomic Theory regarding the composition of compounds?

Chemical compounds are formed when atoms of different elements combine in fixed ratios. Signup and view all the answers

Which of the following is correctly named according to the rules of binary covalent compounds?

Diphosphorus pentoxide for P2O5 Signup and view all the answers

Which statement regarding Dalton's atomic theory is incorrect?

Atoms are made of smaller particles called protons and neutrons Signup and view all the answers

What does the law of definite proportion imply about a compound?

A compound always contains the same relative amounts of its elements by mass. Signup and view all the answers

What is the appropriate naming convention when naming acids that do not contain oxygen?

Using the prefix hydro- and suffix -ic Signup and view all the answers

What characterizes a molecule formed by covalent bonds?

It forms by sharing electrons between atoms Signup and view all the answers

Which of the following compounds is an example of an acid?

HCl Signup and view all the answers

What does Dalton's Atomic Theory state about atoms in a chemical reaction?

Atoms are restructured but remain unchanged. Signup and view all the answers

Which law describes the ratio of the masses of the second element that combine with 1 gram of the first element?

Law of Multiple Proportions Signup and view all the answers

Which prefix indicates the presence of four atoms in a compound?

tetra- Signup and view all the answers

What is the correct name for the compound Mg(NO3)2?

Magnesium nitrate Signup and view all the answers

According to early chemistry practices, what was a significant focus of alchemists?

Converting base metals into gold Signup and view all the answers

What was one of the primary contributions of Robert Boyle to chemistry?

He created the first experimental definition of an element. Signup and view all the answers

Study Notes

Chapter 2: Atoms, Molecules, and Ions

This chapter covers the fundamentals of atoms, molecules, and ions, including their history and modern understanding.

Section 2.1: The Early History of Chemistry

Greeks were the first to attempt to explain chemical changes.
Alchemy dominated for 2000 years, with several elements being discovered and mineral acids prepared.
Robert Boyle was a pivotal figure, performing quantitative experiments and developing the first experimental definition for an element.

Section 2.2: Fundamental Chemical Laws

Law of Conservation of Mass (Lavoisier): Mass is neither created nor destroyed in a chemical reaction.
Law of Definite Proportion (Proust): A given compound always contains exactly the same proportion of elements by mass.
Law of Multiple Proportions (Dalton): When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can be reduced to small whole numbers.

Section 2.3: Dalton's Atomic Theory

Dalton's Atomic theory (1808):
- Each element is made up of tiny particles called atoms
- The atoms of a given element are identical, but the atoms of different elements are different in some fundamental way.
- Chemical compounds are formed when atoms of different elements combine with each other. A given compound always has the same relative numbers and types of atoms.
- Chemical reactions involve reorganization of the atoms—changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction.

Section 2.4: Early Experiments to Characterize the Atom

J. J. Thomson (1898-1903):
- Postulated the existence of negatively charged particles (electrons) using cathode-ray tubes.
- Determined the charge-to-mass ratio of an electron.
- The atom must also contain positive particles to balance the negative charge of electrons.
Ernest Rutherford (1911):
- Explained the nuclear atom.
- The atom has a dense center of positive charge called the nucleus.
- Electrons travel around the nucleus at a large distance relative to the nucleus.

Section 2.5: The Modern View of Atomic Structure

The atom contains:
- Electrons: negatively charged, found outside the nucleus.
- Protons: positively charged, found in the nucleus, with a magnitude of charge equal to the electron's negative charge.
- Neutrons: no charge, found in the nucleus, with a mass virtually the same as a proton.
The nucleus is:
- Small compared to the overall size of the atom.
- Extremely dense, accounting for almost all of the atom's mass.
Isotopes: Atoms with the same number of protons but different numbers of neutrons. They show almost identical chemical properties because the chemistry of an atom is due to its electrons. Most elements contain mixtures of isotopes.
Isotopes are identified by:
- Atomic Number (Z): the number of protons.
- Mass Number (A): the number of protons plus the number of neutrons.

Section 2.6: Molecules and Ions

Chemical Bonds:
- Covalent Bonds: Bonds form between atoms by sharing electrons. The resulting collection of atoms is called a molecule.
- Ionic Bonds: Bonds form due to the attraction between oppositely charged ions.
  - Ion: an atom or group of atoms with a net positive or negative charge.
  - Cation: a positive ion; lost electron(s).
  - Anion: a negative ion; gained electron(s).

Section 2.7: An Introduction to the Periodic Table

Metals vs. Nonmetals: A key classification of elements.
Groups/Families: Vertical columns of elements with similar chemical properties.
Periods: Horizontal rows of elements.

Section 2.8: Naming Simple Compounds

Binary Compounds: Compounds composed of two elements (ionic or covalent).
Binary Ionic Compounds (Type I): The cation is named first, followed by the anion. Monatomic cations take their name from the parent element. Monatomic anions have the element root with -ide added. Examples: KCl (Potassium chloride), MgBr₂ (Magnesium bromide), CaO (Calcium oxide).
Binary Ionic Compounds (Type II): Metals that can form more than one positive ion. The charge of the metal cation must be specified using a Roman numeral. Examples: CuBr (Copper(I) bromide), FeS (Iron(II) sulfide), PbO₂ (Lead(IV) oxide).
Polyatomic Ions: Ions containing multiple atoms. Their names need to be memorized. Examples: NaOH (Sodium hydroxide), Mg(NO₃)₂ (Magnesium nitrate), (NH₄)₂SO₄ (Ammonium sulfate).
Binary Covalent Compounds (Type III): Formed between two nonmetals. The first element is named using its full element name, and the second element is named as an anion, using prefixes to indicate the number of atoms present. Examples: CO₂ (Carbon dioxide), SF₆ (Sulfur hexafluoride), N₂O₄ (Dinitrogen tetroxide).
Acids: Molecules with one or more hydrogen ions (H⁺) attached to an anion. If the anion does not contain oxygen, the acid is named with the prefix "hydro-" and the suffix "-ic." If the anion contains oxygen:
- The suffix "-ic" is added if the anion name ends in "-ate."
- The suffix "-ous" is added if the anion name ends in "-ite." (e.g., HNO₃ (Nitric acid), H₂SO₄ (Sulfuric acid), HNO₂ (Nitrous acid), H₂SO₃ (Sulfurous acid).

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Test your knowledge on the basics of chemical nomenclature and atomic theory with this quiz. Explore questions about acids, isotopes, and the historical contributions to atomic theory. Perfect for students reviewing Chapter 6 in their chemistry course.