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Chem 145 exam 2
| Question | Answer |
|---|---|
| Which has the larger radius - oxygen atom or oxide ion? | Oxide ion |
| Which has the larger radius - calcium atom or calcium ion? | Calicum atom |
| Name a main group element which is likely to form an anion. | Ca (Calcium) |
| Typical charge on a postassium ion? | +1 |
| The total number of electrons in a +1 charge potassium ion. | 18 |
| List and element which is likely to form an ion with a 2+ charge. | Ca (Calcium) |
| Which has the larger radius - magnesium ion or fluoride ion? | Fluoride ion |
| Which compound would you predict to have the higher melting point: CaO or K20? | CaO |
| List the following atoms in order of smallest to largest atomic radii: K Li C N Ca | N C Li Ca K |
| Which one of these has the highest first ionization energy? K Li C N Ca | N (Nitrogen) |
| What is the reason for the large second ionoization energy for potassium? | Because it is stable after the 1st ionization. For the 2nd ionization you would be taking from the core which is much closer to the nucleus (which has a + charge and is pulling all the electrons in tightly) |
| True or False: Na+ has a higher ionization energy than does Na. | True |
| True or False: Sodium atoms and sodium ion are approximately the same size. | False. They are not the same size. The ions are larger that then atom |
| True or False: Atomic radii decreases going across the periodic table from Li to Ne. | True |
| True or False: O has a larger radius than 0(-2 charge). | False. The atom is always smaller than the anion. |
| True or False: It is harder to remove the second electron from Mg than it is to remove the first electron. | True |
| The relationship of c vs lamda in the light equation is : linear, reciprocal, exponential or none. | There is none. C is a constant (the speed of light) and will not change |
| The relationship of E vs c in the light equation is : linear, reciprocal, exponential or none | There is none. C is a constant (the speed of light) and will not change |
| The relationship of v vx lamda in the light equation: linear, reciprocal, exponential or none. | Reciprocal |
| The relationship of h vs lamda in the light equation is: linear, reciprocal, exponential or none. | There is none. H is a constant (Plank's constant) and will not change |
| Predict the formula of the ionic compound that would be formed by the combination of a sodium ion and a fluroide ion. | NaF |
| Predict the formula of the ionic compound that would be formed by the combination of a calcium ion and a hydroxide ion. | Ca(OH)2 |
| Predict the formula of the ionic compound that would be formed by the combination of an aluminum ion and a carbonate ion. | Al2(C03)3 |
| What is the formula for copper (I) bromide and is it ionic or molecular? | CuBr and Ionic |
| What is the formula for copper (II) bromide and is it ionic or molecular? | CuBr2 and Ionic |
| Based on the guidelines for naming oxyanions in a series, name the following: BrO; BrO2; BrO3; and BrO4 | hypobromite; bromite; bromate; perbromate |
| What is the correct name for the formula SeCl4 and is it ionic or molecular? | Selenium Tetrachloride and moleuclar |
| When dissolved in water will potassium sulfide be an electrolyte? | Yes - ionic compounds when dissolved in water become strong electrolytes |
| Which has the higher meling point - calcium oxide or lithium chloride? | Calcium oxide |
| Which is more likely to be water-soluble - calcium oxide or lithium chloride? | Lithium chloride |
| True or False: Atomic radii decreases going across the periodic table from Li to Ne. | True |
| True or False: Sodium atoms have smaller radii than do potassium atoms | True |
| True or False: The transition metals in a period hall have approximately the same atomic size. | True |
| What is the molar mass of calcium dihydrogen phosphate? | 234.052 g/mol |
| Name an example of a strong electrolyte. | NaCl |
| The radius of a cation is always _______ than its corresponding atom from which it is derived. | smaller |
| List and element with a larger first ionization energy than oxygen. | Ne (neon) |
| Why is there no third ionization energy for helium? | The electrons are all gone |
| Give the molar mass of aluminum dichromate. | 701.96 g/mol |
| How many grams of carbon are in a 100 gram sample of carbon disulfide? | 1-C=12; 2-S=64.12 totaling 76.12 g/mol. 12/76.12 x 100 = 15.76% grams of carbon |
| True or False: F has a smaller first ionization energy than does Li. | False. Li has a smaller first ionization energy than does F. F has the largest because it's almost stable - it doesn't want to lose any more electrons |
| True or False: Kr has a smaller radius than K | True |
| True or False: It is harder to remove the first electron from postassium than it is to remove the second electron. | False - it is much harder to remove the second electron from potassium |
| What are the steps you need to take when drawing a correct Lewis structure? | 1)Determine the correct formula 2)Add up the valence e- 3)Draw a skeleton structure w/ shared pair of e- btween each 4)Place e- about the terminal atoms 5)Any left over electrons go around the central atom 6)if central has too few, terminal atoms share e- |
| In a couple sentences, explain how one can generally predict whether or not a given ionic compound will be water-soluble. | Ionic compounds with a +1 or -1 charge are generally considered to be water-soluble. Ionic compounds with a +2/-2; +3/-2; +3/-3; +2/-3 are likely to be considered not water-soluble |
| Which of these is not a typical property of ionic compounds: generally high melting points; they conduct electricity as solids; they consist of anions and cations | Ionic compounds DO NOT conduct electricty as solids |
| Which has more atoms - 54.0 grams of aluminum or 54.0 grams of silicon? | 54.0 grams aluminum |
| Give an example of a free radical. | NO - it is actually a "stable" free radical |
| Which of these single bonds has the shortest bond length: C-O; C-F; C-N; C-C; C-B | C-F |
| List a formula of a compound that contains covalent bonds. | H2O |
| Breaking of which O to O bond requires a more powerful photon, the one found in O2 or O3? Explain your reasoning. What's the difference between the O to O bonds of these molecules? | O2 has a stronger bond and requires a more powerful photon. O3 bond resonates its bonds while O2 does not. |
| List a molecule or polyatomic ion that contains a free pair of electrons. | NH3 |
| Give the formula for calcium acetate. | Ca(CH3COO)2 |
| What is atomic radii? | The size of an atom |
| What is a cation? | An ion with a postivie charge |
| What is ionization energy? | The energy needed to remove a mole of electrons from a mole of atoms in the gas phase |
| What is a binary compound? | A molecular compound whose molecules contains atoms of only two elements |
| What is a molecular compound? | A compound composed of atoms of two or more electrons chemically combined in molecules |
| What are ions? | An atom or group of atoms that has lost or gained one or more electrons so that it is no longer electrically neutral. |
| What is a polyatomic ion? | An ion consisting of more than one atom |
| What is a crystal lattice? | The ordered, repeating arrangement of ions, molecules, or atoms in a cystalline solid |
| What is an electrolyte? | A substance that ionizes or dissociates in water to form an electrically conducting solution |
| What is a formula unit? | The simplest cation-anion grouping representeed by the formula of an ionic compound; also the united represented by any formula |
| What is molar mass? | The mass in grams of 1 mol of atoms, molecules, or formula units of one kind, numerically equal to the atomic or molecular weight in amu |
| What is a moleuclar compound? | A compound composed of atoms of two or more elements chemically combined in molecules |
| What are ionic hydrates? | Ionic compounds that incorporate water molecules in the ionic crystal lattice |
| What is an empirical formula? | A formula sharing the simplest possible ratio of atoms of elements in a compound |
| What is a covalent bond? | Interacive attraction resuling from the sharing of electrons between two atoms |
| What is bond energy? | The change in enthalopy when a mole of chemical bonds of a given type is broken, separting the bonded atoms, the atoms and molecules must be in the gas phase |
| What are non-bonding pairs AKA lone-pair electrons? | Paired valence electrons unused in bond formation also called non-bonding pairs |
| What is bond length? | The distance between the centers of the nuclei of two bonded atoms |
| What is the definition of endothermic? | A process in which thermal energy must be transferred into a thermodyamic system in order to maintain constant temp |
| What are isomers? | Compounds that have the same molecular formula but have different arrangements of atoms |
| What are free radicals? | A highly reactive atom, ion or molecule that contains one or more unpaired electrons |
| What are cis-iomers? | The isomer in which two like subsituments are on the same side of a carbon-carbon double bond, the same side of a ring of carbon atoms, or the same side of a complex ion |
| What are coordinate covalent bonds? | A chemical bond in which both of the two electrons forming the bond were originally associated with the same one of the two bonded atoms |
| What is a complex ion? | An ion with several molecules or ions connected to a central metal ion by coordinate covalent bonds |
| What are lignands? | Atoms, molecules or ions bonded to a central atom, such as the central metal ion in a coordination complex |
| What is a coordination number? | The number of coordinate covalent bonds between ligands and a central metal ion in a complex ion |
| What is the definition of electronegativity? | A measure of the ablility of an atom in a molecules to attract bonding electrons to itself |
| What is a polar covalent bond? | A covalent bond between atoms with different electrons, activities, bonding electrons are shared unequally between the atoms |
| Of the following, SO2/CO2/O3/NO2, list any/all of the following molecules that can be classified as a free radical. | NO2 is the only one with an odd number of electrons |
| Which is the most electronegative atom of the following: C, N, Si, P | N (nitrogen) |
| List a compound that contains polar covalent bonds. | CH3OH |
| For each molecule of carbon monoxide, which atom(s) has (have) a partical plus charge? | C (carbon) - because O is more polar and would have the negative charge |
| Of the following single bonds----> C-C, C-O, C-Cl, C-F, C-N which bond is the longest? | C-Cl |
| Of the following single bonds---> C-C,C-O, C-Cl, C-F, C-N which bond is the most polar? | C-F |
| Of the following single bonds---> C-C, C-O, C-Cl- C-F, C-N which bond is the least polar? | C-C |
| Which of the following molecules is least likely to exist - PF5, IF5, NF5, SbF5 - explain your reasoning. | NF5 - Nitrogen is in period 2 and cannot form 5 bonds - it cannot tap inot an empty D shell |
| Although oxygen exists as O2 and O3, nitrogen only occurs as N2. Account for this fact (explain why N3 is nonexistent) | It would have an odd number of electrons making it a free radial and highly reactive. The electrons would total 15 |
| Name an element that has very high electronegativity | F (fluorine) has the highest |
| Why does fluorine have a very high electronegativity? | It is a very small atom and the shared pair has very limited shielding to the F nucleus |
| When an element is said to have high electronegativity, what does that mean? | That is is the most polar (ie most negative) in the molecule, pulling others (their electrons) towards itself |
| Lithium fluoride (LiF), methane (CH4), and water all have approximately the same molar mass. Whic of these three is the ionic compound? | Lithium fluoride (LiF) |
| Lithium fluoride (LiF), methane (CH4) and water all have approximately the same molar mass. Which of these three is the polar-compound? | Water |
| Lithium fluoride (LiF), methane (CH4) and water all have approximately the same molar mass. Which of these three is the non-polar compound? | Methane (CH4) |
| True or False: A coordinate bond is formed by the donation of a pair of electrons from a ligand to the metal ion. | True |
| True or False: the number of ligands must equal the charge present on the metal ion. | False - Ligands can be neutral or negatively charged. They do not have to equal the charge of the metal ion |
| True or False: A complex ion is defined as an ion with several molecules or ions attached to a central metal ion by coordinate covalent bonds. | True |
| True or False: A ligand can be either neutral or negatively charged. | True - a ligand can never be positively charged because then it would repel the central metal |
| True or False: Counter ions balance the charge of the complex ion in a coordination compound. | True |
| Order the C-C or C-O bonds of C2H2, C2H4, CO, and C2H4 from longest to shortest length. | C2H6, C2H4, C2H2, CO - CO also has the strongest bond since it is the shortest and a C-O bond is stronger/shorter than a C-C bond |
| What is NH4 and what is its charge? | Ammonium and +1 |
| What is OH and what is its charge? | Hydroxide and -1 |
| What is HSO4 and what is its charge? | Hydrogen sulfate and -1 |
| What is CH3COO and what is its charge? | Acetate and -1 |
| What is ClO and what is its charge? | Hypochlorite and -1 |
| What is ClO2 and what is its charge? | Chlorite and -1 |
| What is ClO3 and what is its charge? | Chlorate and -1 |
| What is ClO4 and what is its charge? | Perchlorate and -1 |
| What is NO2 and what is its charge? | Nitrite and -1 |
| What is NO3 and what is its charge? | Nitrate and -1 |
| What is MnO4 and what is its charge? | Permanganate and -1 |
| What is H2PO4 and what is its charge? | Dihydrogen phosphate and -1 |
| What is CN and what is its charge? | Cyanide and -1 |
| What is HCO3 and what is its charge? | Hydrogen carbonate (bicarbonate - old name)and -1 |
| What is CO3 and what is its charge? | Carbonate and -2 |
| What is HPO4 and what is its charge? | Monohydrogen phosphate and -2 |
| What is Cr2O7 and what is its charge? | Dichromate and -2 |
| What is S2O3 and what is its charge? | Thiosulfate and -2 |
| What is SO3 and what is its charge? | Sulfite and -2 |
| What is SO4 and what is its charge? | Sulfate and -2 |
| What is C2O4 and waht is its charge? | Oxalate and -2 |
| What is PO4 and what is its charge? | Phosphate and -3 |
Created by:
juret7674