Molecular Bonding and Chemical Composition
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Molecular Bonding and Chemical Composition

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Questions and Answers

Which type of substance cannot be separated into simpler substances?

  • Solution
  • Mixture
  • Compound
  • Element (correct)

    • Saltwater is a homogeneous mixture.

    True

    What is the chemical formula for sodium chloride?

    NaCl

    The term used for a substance formed when two or more elements chemically combine is called a __________.

    <p>compound</p> Signup and view all the answers

    Match the following terms with their definitions:

    <p>Element = A pure substance that cannot be broken down Mixture = Combination of two or more substances Compound = Substance formed from two or more elements Solution = Homogeneous mixture of two or more substances</p> Signup and view all the answers

    Which of the following describes a heterogeneous mixture?

    <p>Consists of two or more phases</p> Signup and view all the answers

    All compounds are considered mixtures.

    <p>False</p> Signup and view all the answers

    What type of bond is responsible for the formation of compounds?

    <p>covalent or ionic bond</p> Signup and view all the answers

    A __________ is a substance that contains only one kind of atom.

    <p>element</p> Signup and view all the answers

    What is the state of matter where molecules are closely packed together but can still move around each other?

    <p>Liquid</p> Signup and view all the answers

    What term describes a combination of contradictory words?

    <p>Oxymoron</p> Signup and view all the answers

    A polytomous variable is treated as a single unit.

    <p>False</p> Signup and view all the answers

    What is the opposite of a counterpart?

    <p>Antonym</p> Signup and view all the answers

    An example of a __________ would be 'deafening silence'.

    <p>oxymoron</p> Signup and view all the answers

    Match the terms with their definitions:

    <p>Oxymoron = A figure of speech juxtaposing contradictory terms Polytomous = Having multiple categories Counterpart = A person or thing that corresponds to another Bionic = Having artificial body parts</p> Signup and view all the answers

    What type of bonding occurs when atoms combine.?

    <p>Covalent Bonding</p> Signup and view all the answers

    Carbon monoxide is an example of a compound formed by covalent bonding.

    <p>True</p> Signup and view all the answers

    Which of the following is a use of the term 'bionic'?

    <p>Referring to artificial body enhancements</p> Signup and view all the answers

    All terms mentioned are related to literature.

    <p>False</p> Signup and view all the answers

    What is the chemical formula for water?

    <p>H2O</p> Signup and view all the answers

    What can be treated as one in terms of categorization?

    <p>Unit</p> Signup and view all the answers

    In covalent bonding, atoms share ______ to achieve a stable electron configuration.

    <p>electrons</p> Signup and view all the answers

    Match the following terms with their descriptions:

    <p>Covalent Bonding = Sharing electrons between atoms Ionic Bonding = Transfer of electrons between atoms Stable Structure = Atoms held together with minimal energy Electron Shell = Region around the nucleus containing electrons</p> Signup and view all the answers

    How many electrons are available in the outermost energy level for elements in group 18?

    <p>8</p> Signup and view all the answers

    All elements can form compounds through covalent bonding.

    <p>False</p> Signup and view all the answers

    What general trend does nature exhibit regarding energy and bonding?

    <p>Nature tends to take the path of least resistance.</p> Signup and view all the answers

    Chlorine has a tendency to gain electrons to achieve a ______ electron configuration.

    <p>stable</p> Signup and view all the answers

    What type of elements combine to form ionic bonds?

    <p>A metal and a nonmetal</p> Signup and view all the answers

    Stable structures are formed when atoms are far apart.

    <p>False</p> Signup and view all the answers

    What is the role of outermost electrons in bonding?

    <p>They are involved in forming bonds between atoms.</p> Signup and view all the answers

    The chemical formula for carbon dioxide is ______.

    <p>CO2</p> Signup and view all the answers

    Match the elements to their classification:

    <p>Carbon = Nonmetal Sodium = Metal Chlorine = Nonmetal Iron = Metal</p> Signup and view all the answers

    What is the charge of the sulfate anion?

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

    The nitrate ion (NO3-) has a 2- charge.

    <p>False</p> Signup and view all the answers

    What is the charge of the hydroxide ion (OH-)?

    <p>1-</p> Signup and view all the answers

    The chemical formula for dichromate is __________.

    <p>Cr2O7</p> Signup and view all the answers

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

    <p>Nitrate</p> Signup and view all the answers

    Match the following ions with their charges:

    <p>Sulfate = 2- Nitrate = 1- Hydroxide = 1- Dichromate = 2-</p> Signup and view all the answers

    The chloride ion carries a 1- charge.

    <p>True</p> Signup and view all the answers

    How many oxygen atoms are in a sulfate ion?

    <p>4</p> Signup and view all the answers

    What does the arrangement of the periodic table allow you to determine?

    <p>The placement of cations and anions based on their values</p> Signup and view all the answers

    The total negative charge on an ionic compound must equal zero.

    <p>True</p> Signup and view all the answers

    Name the cation present in Sodium Fluoride.

    <p>Sodium</p> Signup and view all the answers

    Beryllium produces _____ when combined with fluoride.

    <p>Beryllium Fluoride</p> Signup and view all the answers

    Match the following ionic compounds with their formulas:

    <p>Lithium Fluoride = LiF Magnesium Oxide = MgO Calcium Nitride = Ca3N2 Sodium Chloride = NaCl</p> Signup and view all the answers

    Which formula represents Copper (II) Oxide?

    <p>CuO</p> Signup and view all the answers

    The name of the compound K2O is Potassium Oxide.

    <p>True</p> Signup and view all the answers

    What is the common charge of cations formed by Group 1 elements?

    <p>+1</p> Signup and view all the answers

    When naming covalent compounds, the prefix 'di-' indicates _____ atoms of that element.

    <p>two</p> Signup and view all the answers

    Match the following cations with their charges:

    <p>Na+ = Sodium Mg2+ = Magnesium Ca2+ = Calcium Fe3+ = Iron</p> Signup and view all the answers

    What is a key property of metal ions in ionic compounds?

    <p>They tend to lose electrons</p> Signup and view all the answers

    The formula for Sodium Nitride is NaN3.

    <p>False</p> Signup and view all the answers

    Identify the anion in the compound Iron (III) Chloride.

    <p>Chloride</p> Signup and view all the answers

    Carbon Dioxide is represented by the formula _____ .

    <p>CO2</p> Signup and view all the answers

    Match the following transition metals with their common oxidation states:

    <p>Copper (I) = Cu+ Iron (II) = Fe2+ Lead (IV) = Pb4+ Manganese (II) = Mn2+</p> Signup and view all the answers

    What is the proper name for the compound with the formula CaF2?

    <p>Calcium Fluoride</p> Signup and view all the answers

    Study Notes

    Molecular Bonding

    • Atoms combine to form elements or compounds
    • Atoms form stable structures when they come close together
    • Nature tends to take the path of least resistance
    • Ionic bonding occurs between metals and non-metals
    • Covalent bonding occurs between non-metals
    • All metals have 1-8 available electrons in their outer most energy level
    • All non-metals have 1-8 available electrons in their outer most energy level
    • LenC refers to the number of electrons in the outer most energy level (n)
    • Elements in group 1 & 2 tend to lose electrons
    • Elements in group 13, 15, 16, & 17 tend to gain electrons

    Chemical Composition

    • Pure substances have consistent composition and properties
    • Mixtures combine different substances with variable compositions
    • Elements are pure substances that cannot be broken down further
    • Compounds combine multiple elements with a fixed ratio and unique properties
    • Heterogeneous mixtures have uneven properties
    • Homogeneous mixtures have uniform properties

    States of Matter

    • Molecules are groups of 2 or more atoms bonded together
    • Atomic elements consist of single atoms
    • At room temperature, Noble gas elements exist as gases
    • Diatomic elements exist in multiple states of matter at room temperature: oxygen, nitrogen, fluorine, bromine, iodine
    • Solid - Molecules closely packed, fixed position
    • Liquid - Molecules less tightly packed, move more freely
    • Gas - Molecules move freely, no fixed position

    Ionic Compounds

    • Ionic compounds consist of a metal cation and a non-metal anion
    • Cations (+) are positively charged ions
    • Anions (-) are negatively charged ions
    • The total charge of the positive and negative ions in a compound must equal zero
    • Ionic compounds are organized in a 3D lattice structure

    Naming Ionic Compounds

    • The name of the metal comes first, followed by the name of the non-metal
    • The name of the non-metal ends in "ide"
    • If a metal can form multiple ions, the charge is written in parentheses after the metal name
    • Example: Iron (II) chloride (FeCl2)
    • Example: Iron (III) chloride (FeCl3)

    Naming Covalent Compounds

    • Start with the name of the element further left on the periodic table
    • The name of the element further right on the periodic table ends in "ide"
    • Use Greek prefixes to indicate the number of atoms of each element

    Binary Compounds

    • Binary compounds consist of two elements
    • The number of each element must balance out the positive and negative charges
    • Common examples include: CO, P2O5, KCI, Mg(NO3)2, SO2, CaCO3, NaHCO3, NH4Cl

    Cations and Anions

    • Cations are positively charged ions
    • Anions are negatively charged ions
    • The charge of an ion is determined by the number of protons and electrons it contains
    • Protons carry a positive charge, while electrons carry a negative charge
    • Ions are formed when an atom gains or loses electrons

    Chemical Formulas

    • The chemical formula of a compound describes the types and quantities of atoms that make up the compound
    • The subscript numbers in a chemical formula indicate the number of atoms of each element in the compound
    • Example: The formula for water is H2O, indicating that each water molecule contains two hydrogen atoms and one oxygen atom.

    Common Ions

    • Some common ions:
      • $SO_4^{2-}$ Sulfate Anion
      • $CO_3^{2-}$ Carbonate Anion
      • $Cr_2O_7^{2−}$ Dichromate anion
      • $NO_3^{1−}$ Nitrate anion
      • $NO_2^{1−}$ Nitrite anion
      • $OH^{1-}$ Hydroxide anion
      • $ClO_2^{1−}$ Chlorite anion
      • $ClO_3^{1−}$ Chlorate anion
      • $NH_4^{+}$ Ammonium cation

    Neutral Charge

    • The net charge of a neutral compound is always zero
    • This means that the total number of positive charges from cations must equal the total number of negative charges from anions

    Example

    • To determine the charge of an iron cation, we can use the chemical formula for iron(III) oxide, which is $Fe_2O_3$
    • The oxide anion has a charge of -2
    • There are three oxide anions in the formula, giving a total negative charge of -6
    • Since the compound is neutral, the total positive charge must also be +6
    • There are two iron cations, so each iron cation must have a charge of +3
    • The charge of the iron cation in this example is +3.

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    Description

    This quiz covers essential concepts related to molecular bonding and chemical composition. It explores how atoms combine to form elements, compounds, and mixtures, including the distinctions between ionic and covalent bonding. Test your understanding of the properties of pure substances and the behavior of metals and non-metals in bonding.

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