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Questions and Answers
What is the charge of an anion?
Which of the following correctly identifies the number of electrons in a cation?
Which of the following statements about metalloids is true?
How many nuclei are contained in a polyatomic molecule?
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What is the correct classification of Na+?
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How many protons and electrons are in 34 Se 2-?
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What is the definition of a diatomic molecule?
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Which of the following is an example of a polyatomic ion?
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What is the main concept of Dalton's Atomic Theory regarding elements?
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What is the correct relationship between mass number and atomic number?
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How are isotopes defined?
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What is true about the nuclei of atoms?
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How many neutrons are present in the isotope 146C?
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What does the atomic number (Z) represent in an atom?
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What is the correct nomenclature for the compound represented by the formula CO?
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Which of the following acids is correctly named based on the anion present?
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What happens to atoms during a chemical reaction according to Dalton's Atomic Theory?
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What is the chemical formula for diphosphorus pentasulfide?
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Which particle in the nucleus has a negligible mass compared to protons?
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Identify the formula for potassium dihydrogen phosphate.
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Which of the following compounds contains hydroxide ions when dissolved in water?
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What type of compound is NaOCl commonly known as?
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Which of the following correctly identifies the nature of the compound CsClO4?
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What is the correct name for the anion SO4^2-?
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What must the sum of the charges on the cation(s) and anion(s) in an ionic compound formula equal?
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Considering binary ionic compounds, how is a monatomic anion named?
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What is the correct name for the ionic compound CaBr2?
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How are transition metals that can form multiple positive ions specified in their compound names?
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What is the formula for the compound formed between aluminum and oxygen?
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What is the correct name for the ionic compound FeCl2?
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Which of the following ions is a polyatomic ion?
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What distinguishes Type II binary ionic compounds from Type I?
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What is the correct unbalanced equation for the reaction of hydrogen and chlorine gas to form hydrochloric acid?
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In balancing the equation for the formation of water from hydrogen and oxygen, what is the balanced form?
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When balancing the equation FeO(s) + O2(g) Fe2O3(s), what is the sum of the coefficients in standard form?
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Which of the following statements best represents the law of conservation of mass as it relates to chemical reactions?
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What is the proper mechanism for balancing a chemical equation by inspection?
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In balancing the reaction CaO + C CaC2 + CO2, which of the following is incorrect?
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Which of these conditions must be true for a chemical equation to be considered balanced?
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Which of the following statements about physical states in chemical equations is true?
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Study Notes
Dalton’s Atomic Theory
- Elements are composed of atoms. All atoms of the same element are identical, with the same size, mass, and chemical properties. Different elements have different atoms.
- Compounds are made of different types of atoms. One compound will always have the same ratio of each type of atom.
- Atoms are not created or destroyed in chemical reactions. Only rearranged.
The Structure of the Atom
- Atoms have a positive nucleus containing most of the atom's mass.
- The nucleus is surrounded by negatively charged electrons.
Nuclear Structure; Isotopes
- A proton is a nuclear particle with positive charge and is heavier than an electron.
- The atomic number (Z) is the number of protons in the nucleus.
- A neutron is a nuclear particle with almost the same mass as a proton but no charge.
- An element is identified by its atomic number.
- The mass number (A) is the total number of protons and neutrons.
- Isotopes are atoms of the same element, with the same atomic number, but different mass numbers (different number of neutrons).
Metals, Nonmetals, and Metalloids
- Metals are lustrous, good conductors of heat and electricity.
- Nonmetals are not metallic. They are usually brittle in their solid form.
- Metalloids have properties of both metals and nonmetals, and are often semi-conductors.
Molecules
- A molecule is a group of two or more atoms held together by chemical bonds.
- A diatomic molecule has two atoms. Example: H2, O2, N2, F2, Cl2, Br2, I2.
- A polyatomic molecule has more than two atoms. Example: H2O, NH3, CO2
Ions
- An ion is an atom or group of atoms with a positive or negative charge.
- A cation is a positively charged ion formed when a neutral atom loses electrons.
- An anion is negatively charged ion formed when a neutral atom gains electrons.
- A monatomic ion is a single atom with a charge. Example: Na+, Cl-.
- A polyatomic ion is a group of atoms with a net charge. Example: OH-, NO3-, SO42-.
Ionic Compounds
- Ionic compounds are made of cations and anions.
- The sum of the charges for each formula unit must equal zero.
Chemical Nomenclature
- Binary Compounds are made of two elements.
- Binary Ionic Compounds (Type 1) are formed from a metal cation and a nonmetal anion.
- Binary Ionic Compounds (Type II) are formed from metals that can have multiple positive charges.
- Polyatomic Ions are groups of atoms with an overall charge.
- Binary Covalent Compounds (Type III) are formed from two nonmetals.
Acids
- Acids produce H+ ions when dissolved in water.
- An acid molecule has one or more H+ ions attached to an anion.
- If the anion doesn't contain oxygen, the prefix hydro- is used, and the suffix -ic is added.
- If the anion contains oxygen, the root name of the anion is used, and the suffix -ic or -ous is added depending on the anion.
Bases
- Bases produce hydroxide ions (OH-) when dissolved in water.
Chemical Equations
- Chemical reactions are represented by chemical equations.
- Reactants are on the left side of the equation.
- Products are on the right side of the equation.
- Atoms are not created or destroyed in chemical reactions, so the same number of atoms on each side of the equation.
- The physical states of compounds can be represented by letters in the chemical equation.
Balancing Chemical Equations
- The coefficients in front of each chemical formula in a balanced equation indicate the number of molecules involved in the reaction.
- The coefficients are adjusted to ensure an equal number of each atom type on both sides.
- Balancing is done by inspection starting with the most complex molecule.
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Description
Test your understanding of Dalton’s Atomic Theory and the structure of the atom in this quiz. Covering key concepts on elements, compounds, and nuclear structure, this quiz will assess your knowledge of atomic particles and isotopes. Perfect for 10th-grade chemistry students!