Breaking bad

<p>Covalent bond (B)</p> Signup and view all the answers

<p>Transfer of electrons from one atom to another. (C)</p> Signup and view all the answers

<p>Ionic compound (C)</p> Signup and view all the answers

<p>Cation, with one positive charge (A)</p> Signup and view all the answers

<p>CO2 (A)</p> Signup and view all the answers

<p>K2S (C)</p> Signup and view all the answers

<p>Iron(III) Oxide (C)</p> Signup and view all the answers

<p>Al::: (C)</p> Signup and view all the answers

<p>-2 (A)</p> Signup and view all the answers

<p>Ammonium ion (A)</p> Signup and view all the answers

<p>Zinc (B)</p> Signup and view all the answers

<p>2+ (B)</p> Signup and view all the answers

<p>Ammonium (B)</p> Signup and view all the answers

<p>HCO3- (C)</p> Signup and view all the answers

<p>Polyatomic ions with names ending in -ite have one less oxygen than those ending in -ate. (A)</p> Signup and view all the answers

<p>Ba(NO3)2 (C)</p> Signup and view all the answers

<p>The word hydrogen is combined with the polyatomic ion's name. (B)</p> Signup and view all the answers

<p>(NH4)2SO4 (C)</p> Signup and view all the answers

<p>They likely end in -ide. (A)</p> Signup and view all the answers

<p>4 (D)</p> Signup and view all the answers

<p>6 (D)</p> Signup and view all the answers

<p>12 (B)</p> Signup and view all the answers

<p>4 (C)</p> Signup and view all the answers

<p>12 (C)</p> Signup and view all the answers

<p>The law of conservation of mass (A)</p> Signup and view all the answers

<p>To adjust the number of molecules involved in the reaction (B)</p> Signup and view all the answers

<p>Because changing the subscript would alter the identity of the element (C)</p> Signup and view all the answers

<p>To balance the number of nitrogen atoms (B)</p> Signup and view all the answers

<p>Diatomic elements must be represented as molecules, not individual atoms, in chemical equations. (A)</p> Signup and view all the answers

<p>Adding coefficients in front of the chemical formulas (A)</p> Signup and view all the answers

<p>Altering the subscripts in the formulas to match the number of atoms. (C)</p> Signup and view all the answers

<p>A + B 🡪 AB (C)</p> Signup and view all the answers

<p>2 H2O 🡪 2H2 + O2 (C)</p> Signup and view all the answers

<p>2PbO2(s) 🡪 2Pb(s) + 2O2(g) (A)</p> Signup and view all the answers

<p>Mg(s) + F2(g) 🡪 MgF2(s) (A)</p> Signup and view all the answers

<p>Single Replacement (A)</p> Signup and view all the answers

<p>N2(g) + O2(g) 🡪 2NO(g) (D)</p> Signup and view all the answers

<p>Decomposition (B)</p> Signup and view all the answers

<p>Zn(s) + CuSO4(aq) 🡪 ZnSO4(aq) + Cu(s) (A)</p> Signup and view all the answers

<p>The replacing element must be more reactive. (B)</p> Signup and view all the answers

<p>Hydrogen ion (D)</p> Signup and view all the answers

<p>AB + CD 🡪 AC + BD (D)</p> Signup and view all the answers

<p>A hydrocarbon reacts with oxygen gas. (D)</p> Signup and view all the answers

<p>First and last ions combine, then the middle ions. (A)</p> Signup and view all the answers

<p>Potassium (A)</p> Signup and view all the answers

<p>Sodium fluoride and chlorine gas (A)</p> Signup and view all the answers

<p>Double replacement reaction (D)</p> Signup and view all the answers

<p>A salt and water. (D)</p> Signup and view all the answers

<p>Hydrogen ($H^+$) and hydroxide ($OH^-$) ions. (C)</p> Signup and view all the answers

<p>Double displacement. (B)</p> Signup and view all the answers

<p>A salt. (B)</p> Signup and view all the answers

<p>$H_2SO_4(aq) + 2KOH(aq) \rightarrow K_2SO_4(aq) + 2H_2O(l)$ (B)</p> Signup and view all the answers

<p>The solution is basic and has a low concentration of hydrogen ions. (C)</p> Signup and view all the answers

<p>Tastes sour. (C)</p> Signup and view all the answers

<p>1000 times (A)</p> Signup and view all the answers

<p>sulfurous acid (A)</p> Signup and view all the answers

<p>Produces hydronium ions ($H_3O^+$). (A)</p> Signup and view all the answers

The number of protons in an atom's nucleus, which determines the element's identity.

Regions around an atom's nucleus where electrons are likely to be found. They represent different energy levels.

Atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight electrons in their outermost shell.

Atoms with different numbers of electrons in their shells. They can be formed by gaining or losing electrons.

Negatively charged ions formed by gaining electrons. They are often nonmetals.

Positively charged ions formed by losing electrons. They are often metals.

A type of chemical bond formed between nonmetals by the sharing of electron pairs.

A type of chemical bond formed between metals and nonmetals through the transfer of electrons, resulting in the formation of ions.

A type of chemical formula that represents the valence electrons of an atom using dots.

A compound formed by the electrostatic attraction between a positively charged cation and a negatively charged anion.

A method used to write the chemical formula of an ionic compound. The charges of the cation and anion are used to determine the subscripts for each element in the formula.

The ability of an atom to attract electrons in a chemical bond.

A positively charged ion formed from a metal that can have multiple possible charges.

A number written in parentheses after a metal's name, indicating the charge of the cation.

A group of atoms that act as a single unit with an overall charge.

A polyatomic ion containing oxygen and another element.

The process of determining the formula of an ionic compound by balancing the charges of the cation and anion.

A method used to balance the charges in ionic compounds by using subscripts to represent the number of each ion needed.

A polyatomic ion containing hydrogen, such as HCO3-, called hydrogen carbonate.

A number written before a chemical formula, indicating the number of molecules or formula units present.

A number written below and to the right of an element symbol, indicating the number of atoms of that element in a molecule or formula unit.

The coefficient in a chemical formula is multiplied by the subscripts of each element in the formula to determine the total number of atoms of each element.

A chemical formula that represents a single molecule or formula unit.

In a chemical formula, if no subscript is present for an element, it is assumed that there is one atom of that element in the molecule or formula unit.

A chemical equation where the number of atoms of each element on the reactant side equals the number of atoms of that element on the product side.

The principle that matter cannot be created or destroyed in a chemical reaction, only transformed.

An equation that shows the reactants and products of a chemical reaction but does not have balanced coefficients.

A chemical reaction involving the breaking and forming of chemical bonds, resulting in a change in the composition of the reactants.

Substances on the left side of a chemical equation that react to form products.

Substances on the right side of a chemical equation that are formed from the reaction of reactants.

A chemical reaction where two or more substances combine to form a single, more complex product.

A chemical reaction where a single compound breaks down into two or more simpler substances.

A reaction where one element replaces another element in a compound.

A reaction where a metal element replaces a metal cation in a compound.

A reaction involving a nonmetal element replacing a nonmetal anion in a compound.

A reaction where two reactants combine to form one product.

A reaction where a single reactant breaks down into two or more products.

A list of elements organized by their reactivity. Elements higher on the list are more reactive.

A chemical reaction where two compounds exchange ions to form two new compounds. The metal and nonmetal in each compound switch partners.

A chemical reaction involving a hydrocarbon reacting with oxygen gas, producing carbon dioxide, water, and heat.

A chemical reaction where a metal reacts with an acid, producing a salt and hydrogen gas.

A reaction where a metal is more reactive than the metal in a compound, causing the more reactive metal to replace the less reactive one in the compound.

A reaction where a nonmetal is more reactive than the nonmetal in a compound, causing the more reactive nonmetal to replace the less reactive one in the compound.

A chemical reaction where an acid and a base react to form a salt and water.

A type of chemical reaction where the positive and negative ions of two reactants switch places to form two new products.

A reaction where hydrogen ions (H+) from an acid combine with hydroxide ions (OH-) from a base to form water (H2O).

Compounds formed in neutralization reactions, often used in everyday products like water softeners and fertilizers.

A measure of the concentration of hydrogen ions (H+) in a solution, indicating its acidity or alkalinity.

A substance that releases hydrogen ions (H+) when dissolved in water, resulting in a pH lower than 7.

A substance that releases hydroxide ions (OH-) when dissolved in water, resulting in a pH higher than 7.

A chemical reaction where an acid and a base react to form a salt and water.

A compound formed when an acid and a base react, often used in many everyday products.