chemistry
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| WHAT ARE THE TWO MAJOR CATEGORIES OF COMPOUNDS ARE | IONIC AND COVALENT COMPOUNDS
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| WHEN ARE CHEMICAL BONDS FORMED | THEY ARE FORMED WHEN VALENCE ELECTRONS ARE TRANSFERRED(IONIC), SHARED(COVALENT) OR MOBILE WITH IN A METAL (METALLIC)
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| IN A MULTIPLE COVALENT(SHARED) BOND HOW MANY PAIRS OF ELECTRONS ARE SHARED BETWEEN TWO ATOMS. | MORE THAN ONE PAIR OF ELECTRONS ARE SHARED BETWEEN TWO ATOMS.
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| UNSATURATED COVALENT (SHARED) COMPOUNDS CONTAIN WHAT TYPES OF BONDS | UNSATURATED COVALENT COMPOUND CONTAIN AT LEAST ONE DOUBLE OR TRIPLE BOND.
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| HOW CAN MOLECULAR POLARITY BE DETERMINED | ITS CAN BE DETERMINED BY THE SHAPE AND DISTRIBUTION OF THAT CHARGE.
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| WHAT HAPPENS WHEN A BOND IS BROKEN | ENERGY IS ABSORBED.
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| WHAT HAPPENS WHEN A BOND IS FORMED. | ENERGY IS RELEASED.
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| HOW DO ATOMS ATTAIN A STABLE VALENCE ELECTRON CONFIGURATION | THEY ATTAIN A STABLE VALENCE ELECTRON CONFIGURATION BY BONDING WITH OTHER ATOMS.
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| WHAT GASES ARE STABLE AND TEND NOT TO BOND | NOBLE GASES
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| name the 6 Noble gases | He, Ne, Ar, Kr, Xe, Rn
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| IN WHAT TERMS CAN PHYSICAL PROPERTIES OF SUBSTANCES BE EXPLAINED | THEY CAN BE EXPLAINED IN TERMS OF CHEMICAL BONDS AND INTERMOLECULAR FORCES.
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| NAME 5 EXAMPLES OF PHYSICAL PROPERTIES OF SUBSTANCES | CONDUCTIVITY, MELTING AND BOILING POINTS , SOLUBILITY AND HARDNESS.
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| YOU CAN EXPLAIN THE PHYSICAL PROPERTIES OF SUBSTANCES BY KNOWING WHAT | BY KNOWING THE INTERMOLECULAR FORCES AND CHEMICAL BONDS OF THE PHYSICAL PROPERTIES.
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| WHAT DOES THE LEWIS STRUCTURE ABLE TO REPRESENT | IT REPRESENTS THE VALENCE ELECTRON ARRANGEMENT IN ELEMENTS, CMPOUNDS AND IONS.
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| WHAT DOES ELECTRONEGATIVITY INDICATE | ELECTRONEGATIVITY INDICATES HOW STRONGLY AN ATOM OF AN ELEMENT ATTRACTS ELECTRONS IN A CHEMICAL BOND.
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| WHAT IS THE ELECTRONEGATIVITY DIFFERENCE BETWEEN TWO BONDED ATOMS USED FOR | IT IS USED TO ASSESS THE DEGREE OF POLARITY IN A BOND.
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| WHAT TEND TO REACT WITH NONMETALS TO FORM IONIC COMPOUNDS | METALS
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| WHAT TENDS TO REACT WITH OTHER NONMETALS TO FORM MOLECULAR (COVELANT) COMPOUNDS | NONMETALS
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| WHAT DOES LEWIS STRUCTURES REPRESENT | IT REPRESENTS THE VALENCE ELECTRON ARRANGEMENT IN ELEMENTS, COMPOUNDS AND IONS.
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| WHAT REACTS WITH NON METALS TO FORM IONIC(SHARED)COMPOUNDS. | METALS
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| IONIC COMPOUNDS CONTAINING POLYATOMIC IONS HAVE WHAT TYPE OF BONDING | BOTH IONIC AND COVALENT BONDING
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| DEMONSTRATE BONDING CONCEPTS USING DOT STRUCTURES, REPRESENTING VALENCE ELECTRONS TRANSFERRED (IONIC) ,SHARED (CONVALENT ) IN A STABLE OCTET. | DRAW THIS
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| DISTINGUISH BETWEEN NONPOLAR AND COVALENT BONDS AND POLAR COVALENT BONDS |
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| TO BE ABLE TO EXPLAIN THE TRANSFER OF ENERGY THAT OCCURS DURING BONDING EXPLAIN WHY DO ATOMS BOND? | FORCES OF ATTRACTION BETWEEN THE PROTONS OF ONE ATOM AND THE ELECTRONS OF ANOTHER ATOM.
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| WHAT TYPE OF ELECTRONS PARTICIPATE IN BONDING | ONLY VALANCE ELECTRONS PARTICIPATE IN BONDING.
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| WHY ARE BONDS FORMED? THEY ARE THE RESULT OF A | CHEMICAL REACTION 1. BUBBLING/ FIZZ COLOR CHANGE ENERGY CHANGE
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| HOW ARE THE BONDS FORMED IN A CHEMICAL REACTION | THROUGH THE EXCHANGE OF ENERGY
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| THROUGH THE EXCHANGE OF ENERGY WHAT IS FORMED IN A CHEMICAL REACTION | BONDS
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| WHAT DOES IT MEAN TO HAVE A SPONTANEOUS BOND FORMATION? | EXOTHERMIC= ENERGY RELEASED
GO FROM HIGH ENERGY (UNSTABLE STATE TO A LOW ENERGY STATE (STABLE STATE)
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| CREATING A BOND CREATES WHAT TYPE OF ENVIRNMENT | STABILITY
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| WHAT HAPPENS DURING SPONTANEOUS BOND FORMATION | ENERGY IS RELEASED WHICH IS EXOTHERMIC
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| DEFINE EXOTHERMIC | ENERGY RELEASED AS A PRODUCT.
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| HOW ARE BONDS FORMED | THROUGH THE EXCHANGE OF ENERGY
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| BONDS ARE FORM DURING EXOTHERMIC CHEMICAL REACTION | ENERGY IS RELEASED AS A PRODUCT
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| A+B->AB+ENERGY IS AN EXAMPLE OF WHAT TYPE OF CHEMICAL REACTION | EXOTHERMIC MEANING ENERGY IS RELEASED AS A PRODUCT
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| 2Na + cl2->2NaCl + heat WHAT ARE THE UNITS OF ENERGY AND HEAT MEASURED IN A + B -> AB + ENERGY | JOULES
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| WHEN YOU HAVE A SPONTANEOUS BOND FORMATION WHAT FORMATION STATE DOES ENERGY RELEASE FROM | IT GOES FROM A STATE OF HIGH ENERGY (UNSTABLE STATE) TO LOW ENERGY (STABLE STATE
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| HOW ARE THESE BONDS BROKEN? | NON SPONTANEOUS BOND BREAKING
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| DEFINE NON SPONTANEOUS BOND BREAKING | ENDOTHERMIC =
WHICH MEANS ENERGY IS CONSUMED IT GOES FROM A LOW ENERGY (STABLE STABILITY) TO A HIGH ENERGY (UNSTABLE)
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| ENDOTHERMIC REACTIONS LIKE MORE ENERGY IS REQUIRED TO BREAK THE STRONGER BOND IN THE REACTANTS THE DIFFERENCE IN ENERGY MUST BE ABSORBED FROM THE SURROUNDINGS FOR THE REACTION TO OCCUR. Potential energy here N2 +O2 -> 2 NO(g) 1 mol N2 1 mol 02 |
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| in an endothermic reaction energy is consumed as a | reactant
more energy is requited to break the stronger bond in the reactants compared to the bonds formed in the reactancts
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| In a Non Spontaneous Bond breaking what type of energy is required to assist in the bond breaking | Endothermic energy which is consumed
and goes from a low energy (stabile state) to high energy(unstable state
ripping 2 + atoms apart requires energy.
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| when is energy consumed as a reactant | during endothermic chemical reactions
energy is consumed as a reactant
(reactants )2 NaCl+ energy -> 2 Na +Cl2 (products)
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| there are two types of interactions elements have: name them | Intramolecular and Intermolecular
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| Intramolecular means? | within
Intranet= school with in a bond( 2atoms)
H- Br
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| what does Intermolecular mean | means between
internet= www.intermolecular
H-CL...
H-CL
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| how to categorize the types of bonds that exist with in compounds ther are many types of bonding with in atoms | ionic
covalent and metallic bonding
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| define Ionic bonds | compounds formed by the transfer of electrons from one atom or polyatomic ion to another
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| in ionic bonds how are compounds formed? | they are formed by the transfer of electrons from one atom or polyatomic ion to another
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| what type of bond would happen if you had metal + non metal bonded | Ionic bond
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| How can you determine ionic compounds | you can determine ionic compounds by the TYPES of elements in your compound. OR
by the greater percent ionic character!!! the closer the electronegativity difference is to four, the greater percent ionic character.!!!!
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| whenti= |
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| the closer the electonegativity difference in the compound is to Four the ...... | greater Ionic Character
differences down to and equal to 1.7 are considered ionic.
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| [AL] 3 3{BR]-1 1.6 -3.0 = *1.4****** still ionic Because its a metal and non metal |
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| what is the excetions to he rule . For ionic compounds? | Polyatomic ions are the exception
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| Polyatomic Ions: Table E consists of | an ion composed of multple ions bonded together
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| Polyatomic ions have what type of bonds | both type of bonds
ionic compounds bonds between N and CL are covalant
NH4CL= ionic compound CL is a Non Metal the bond between Nand cl is covalent (Non metal and Nonmetal
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| define Covalent Bonds | Compounds formed when two or more nonmetals share electrons
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| covalent bonds each bond(line) contain how many electrons | two electrons
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| because of the variation in the number of valence electrons in covalent compounds | covvalent compounds can form multiple bonds
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| what do you call a one dash line in a diagram | Single bond
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| in a diagram what does two dashes/ lines stand for | a double bond
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| How many bonds (electron Pairs) exist between the carbons C=C | 2 bonds =
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| How many electrons are shared between the carbons C=C | 2 pairs 2 electons per pair so 4 electons between the carbons
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| what does three dashes/lines stand for H-C=_H | triple bond
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| How many bonds (electron pairs) exist between the carbons | 3 cause there are 3 lines each line represents a pair 2 electrons per pair
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| what is a Coordinate Covalent Bonds | Covalent Bond in which Both e of the electrons come from the same atom.
Ex- polyatomic ions alone, like NH4
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| define metallic bonding | metalic atoms have few valence electons and have low ionization energies
(easy to lose Valence elctrons)
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| true or false Metallic atoms have few valence electrons and have love ionization energies which make it easy to lose Valence Electrons | True
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| How are the nuclei of metallic atoms arranged? | they are arranged in fixed positions called a crystal lattia
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| define Crystal lattic | is a nuclei of a metalic atom arranged in fixed positions with valence electrons moving freely around them.
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| what is metallic boinding described as | described as the force of attraction between the negativily charged electrons and the positiviely charged nuclei.
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| true or false none of the electons are attached to a particular nucleus in METTALLIC BONDING | TRUE,
METALLIC BONDING IS DESCRIBED AS THE FORCE OF ATTRACTION BETWEEN THE NEGATIVELY CHARGED ELECTRONS AND THE POSITVELY CHARGED NUCLEI.
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| WHAT IS CONSIDERED A SEA OF MOBILE VALENCE ELECTRONS. | METALLIC ATOMS BECAUSE THEY HAVE FEW VALENCE ELECTRONS AND LOW IONIZATION ENERGIES WHICH MAKES IT EASY TO LOOSE ELECTRONS THE NUCLEI IS ARRANGED IN FIXED POSITIONS CALLED CRYSTAL LATTICE WHICH HAVE VALENCE ELECTRONS MOVING FREELY AROUND THEM.
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| DESCRIBE METALLIC BONDING | THE FORCE OF ATTRACTION BETWEEN THE NEGATIVLY CHARGED ELECTRONS AND THE POSITIVELY CHARGED NUCLEI.
NONE OF THE ELECTRONS ARE ATTACHED TO A PARTICULAR NUCLUES. ITS A SEA OF MOBILE VALENCE ELECTRONS.
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| WHAT IS ANOTHER WAY TO CALL A COMPOUND COVALENT? CATEGORIZE COVALENT COMPOUNDS DUE TO POLARITIES | THERE ARE TWO TYPES OF COVALENT MOLECULES
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| NAME THE TWO TYPES OF COVALENT MOLECULES | POLAR MOLECULES(AKA POLAR COVALENT
NON POLAR MOLECULES NON POLAR COVALENT
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| define Metallic bonding | the force of attraction between the NEGATIVELY CHARGED ELECTRONS AND THE POSITIVELY CHARGED NUCLEI.
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| in metallic bonding are the electrons attached to a particular nucleus | No None of the electrons are attached to a particular nucleus.
Its a SEA OF MOBILE VALENCE ELECTRONS
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| WHAT DO YOU CALL THE NUCLEI OF METALLIC ATOMS THAT ARE IN A FIXED POSITION? THAT HAVE VALENCE ELECTRONS MOVING AROUND FREELY. | CRYSTAL LATTICE
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| WHAT IS A CRYSTAL LATTICE | CRYSTALS ARE COMPOSED OF three dimensional patterns. these patterns consist of atoms or groups of atoms in ordered and symmetrical arrangements which are repeated at regular intervels keeping the same orientation to one another. by replacing each group of
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| name the two types of COVALENT Molecules | Polar Molecules(AKA Polar Covalent)
Non Polar Molecules Non Polar Covalent
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| Define Polar Molecules (Polar Covalent) | Asymmetrical- 2 Planes or More
Unequal Sharing of Electrons
2 Atoms on both sides of the Bond/ EN
More than 2 Atoms with Unbonded E- or Lone pairs on Central Atom.
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| What is another way to determine Polarity based on What? | Electronegativity
Remember the Value 1.7? If your electronegativity difference is between
.4 and 1.7 It is Polar Covalent.
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| if your Electronegativity difference is between __ and ___ its POLAR COVALENT. | .4 AND 1.7
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| IN ORDER TO DETERMINE IF SOMETHING IS POLAR COVALENT WHAT DOES THE ELECTRONEGATIVITY DIFFERENCE HAVE TO BE | BETWEEN .4 AND 1.7
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| USING YOUR PERIODIC TABEL DETERMINE THE ELECTRONEGATIVITY OF HCL AND IS IT POLAR COVALENT | YES POLAR COVALENT ELECTRONEGATIVITY IS 1.0
2.2-3.2=1.0
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| IS H20 POLAR | YES 2.2- 3.4 = 1.2 ELECTRONEGATIVITY
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| WHAT IS THE ELECTRONEGATIVITY OF NH3 ? IS IT POLAR? | 2.2- 3.0= .8POLAR
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| DEFINE CHARACTERISITICS OF NONPOLAR MOLECULES(AKA NON POLAR COVALENT) | Symmetrical molecules
equal sharing of molecules
2 Atoms -> same element or EN #'s
More than 2 Atoms BUT with No extra é on central atom
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| draw Cl2 what is the Electronegativity of it | EN = 0
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| draw CC4 what is the Electronegativity whats special about this | EN = 2.6 -3.2 = .6
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| what does your Electronegativity have to be to be NON POLAR COVALENT | IF YOUR ELECTRONEGATIVITY DIFFERENCE IS BETWEEN 0 AND .3 IT IS NON POLAR COVALENT.
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| HOW to classiify types of bonds by their Physical and chemical properties Each type of bond has different _________ | Properties
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| what are the 4 different properties you look at to classify the type of bond you have | Conductivity
Electricity
Melting Point
Boiling Point
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| define Conductivity | its the ability of a substance to allow the flow of ectricity and / or heat
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| define Electricity | Electricity is the Flow of many mobile ELECTRONS or IONS
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| define Melting Point | The temperature at which a substance Melts (Same as Freezing)
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| define Boiling Point | the temperature at which a substance boils.
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| Is an Ionic bond Conductive | on in (aa) form
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| what is the Melt/boining Point of an Ionic bond | High
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| give examples of Ionic bonds | NaCL
CUCL2
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| Molecular bond does it have conductivity | its a NON conductor
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| what is the boiling/ Melt point of a molecular bond | LOW
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| give examples of a Molecular bond that is a Non Conductor and has a low metl /boiling point | C6 H12 02
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| Metallic bonds when are they conductive | when in solid and liquod forms
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| Metallic bonds boil and Meting point what is it High or Low | it has to be at aHIGH TEMP for it to boil or melt
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| give example of Metallic elements | Cu Fe
Copper and Iron
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| Networks are they conductive | Non Conductors
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| Networks what is their Boiling and or Melting point | High temperature needed to boil or melt
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| what are examples of Network elements | diamond ,graphite, SiO2
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| True or False Determining the type of bond will not completely tell us the information about the shapes of compounds? | True
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| what do we use to determine the shapes of compounds | their Lewis Structures , and a simple concept, VSEPR Theory to do just that
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| what does VSEPR stand form | Valence Shell Electron Pair Repulsion Theory
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| what is the VSEPR for? | Valence Shell Electron Pair Repulsion Theory Helps you predict the geometry of individual molecules from é paris on the central Atom
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| what are the Shapes of Covalent Molecules | Linear Line, X2 or Hx
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| what is the compound is the exception to the Linear catagory for Covalent bonds | C02
0=C=O
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| Name the types of shapes covalent molecules can have | Tetrahedral
Pyramidal
Bent
Linear
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| In a Bent shaped Covalent Molecule how are the atoms arranged? H20 H2Se | 3 Atoms are bonded to this Molecule H w/ Group 16
H20
H2Se
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| How are the Atoms arranged on a Pyramidal shaped compounds | 4 atoms bonded
NH3 or PI3 = Nx3 and Px3
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| How many Atoms are arranged on a Tetrahedral | 5 Atoms bonded
example
CCL4 Cx4 Cf4 Cx4 see notes for photos
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| Molecular Symmetry what should you be aware of with these shaped Covalent Bonds?????????????? | Beware there are often POLAR BONDS inside of Non Polar Molecules
Ex CF4 the bond = Polar
Molecule = Non Polar
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| define what a molecule is | a molecue is the smallest particle in a chemical element or compound that has the chemical properties of that element of compound.
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| what are Molecules made up of | Molecules are made up of atoms that are held together by Chemical bonds.
These bonds form as a result of the sharing or exchange of electrons among atoms.
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| what do you call it when two or more atoms form chemical bonds with each other | Molecule
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| Molecules can be simple or complex examples of Molecules N2, O3, CaO , C6 H12 O6 |
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| what is the difference between a molecule and a compound? | a compound is actually a type of molecule A molecule is formed when two or more atoms of an element chemically join together. If the types of ATOMS are different from each other, a COMPOUND is formed.
Not all Molecules are Compounds. since some molecule
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| true or false not all molecules are compounds? | true Not all molecules are compounds, since some moleculres , such as Hydrogen gas or Ozone, consist only of one element or type of ATOM.
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| Examples of Molecules H20 , 02, 03 compound examples NaCL, H20 |
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| true or false the terms molecule and compound mean the same thing and can be used interchangeably. |
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| In Ionic bonds the atoms are bound together by what? Opposites attract | the attraction between oppositely-charged ions. for example Sodium and chloride form together to form an Ionic bond NaCL or Table Salt.
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| Covalent bonds how are the atoms bonded | they are bound by Shared electrons if the electrons are shared equally the bond is said to be Non Polar
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| In Covalent bonds they are formed by sharing electrons If there is an electron Usually an electron is more attracted to one atom than to another this is an unqual |
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| the electrons in a non polar covalent bond are: | shared equally
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| when you have oppositively - charged ions attracted to each other what type of bond do you have | Ionic bond
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| give an example of an ionic bond that we use in our homes every day | NACL
table salt
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| when you have atoms bound by shared electrons what do you call that | covalent bond
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| if the atoms are bound by shared electrons and you have an electron more attracted to one than the other what type of Covalent bond is that | POLAR BECAUSE THEY ARE BOUND TOGETHER BY SHARING OF ELECTRONS CALLING IT COVALENT. BUT SINCE THEY ARNT SHARING ELECTRONS EQUALLY IT NOW BECOMES POLAR
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| WATER H20 IS AN EXAMPLE OF WHAT TYPE OF BOND | POLAR COVALENT
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