AP CHEM EVERYTHING .... YAY
The correct formula for ammonium sulfate is
(NH₄)₂SO₄
The charge on a strontium ion in its ionic compound is
+2
How many of the following are pure compounds? sodium, sugar, oxygen, air, iron
1
7.98 moles of sulfur trioxide molecules contain how many oxygen atoms?
1.44 x 10²⁵
Express the number 178481 in scientific notation
1.78481 x 10⁵
1.8 kilograms contains this many grams
1.8 x 10³
Convert: 92.1 g of CO = _____ molecules of CO
1.98 x 10²⁴
How many protons are in the nucleus of a Mg atom?
12
How many proton, electron, and neutrons, respectively, does ³¹P have?
15, 15, 16
How many moles of Ca atoms are in 613.3 g Ca?
15.30 mol
How many of the following compounds are nonpolar? CBr₂H₂ BH₃ XeCl₄ SF₄ HCl
2
The alkaline earth metals have how many valence electrons?
2
Name the following molecule. CH₃ | CH₃ -- C -- CH₃ | CH₃ -- CH -- CH₂ -- CH -- CH₃ | CH₂ | CH₃ -- CH₂ -- CH₂ -- C -- CH₂ -- CH₂ -- CH | CH₃ -- C -- CH₃ | CH₃ ^^^Depressed bc quizlet is annoying af but just know that the big a** molecule is ------->
2,2,3,5-tetramethyl-7-propyl-7-t-butyldecane
Baking soda and vinegar are mixed in a balloon. A gas is produced, and the balloon expands to a volume of 2.59 L. What is the volume of the balloon is cm³?
2.59 x 10³ cm³
A car tire has a pressure of 39 psi (pounds per square inch). What is the pressure of the tire in atm (atmospheres)? (1 atm=14.70 psi)
2.7 atm
The number of grams in 2.58 mol of sodium carbonate is
273.0 g
CH₃ | CH₃CH₂CHCH₂CH₃
3 - methyl pentane
The number 3.00183 rounded to four significant figures is
3.002
The number 0.00003009 expressed in exponential notation is
3.009 x 10⁻⁵
The number of cubic centimeters (cm³) in 43.0 mL is
43.0 cm³
Calculate the molar mass of a sample if a single molecule weighs 8.90 x 10⁻²³ g.
53.6 g/mol
An atom with 45 protons has a mass number of 100. It must contain how many neurons?
55
Convert: 6.0 mm = ___________ km
6.0 x 10⁻⁶ km
One mole of something consists of _______ units of that substance
6.022 x 10²³
Calculate the mass of 3.53 x 10²⁶ atoms of silver.
6.32 x 10⁴ g
How many atoms are there in 71.9 g of nickel?
7.38 x 10²³
How many protons, electrons, and neutrons, respectively, does ¹⁶O have?
8, 8, 8
What is the mass of 8 atoms of copper in grams?
8.44 x 10⁻²² g
How many millimeters are in 8.63 x 10² centimeters?
8.63 x 10³ mm
How many atoms of calcium are present in 58.2 g of calcium?
8.74 x 10²³
Which of the following exhibit London dispersion forces between molecules? a. HF b. CH₄ c. NH₃ d. H₂O e. All of the above
All of the above
USE THIS CHART: Name / Melting point in K / First Ion. en. in KJ∙mol⁻¹ Lithium / 454 / 519 Sodium / 371 / 494 Potassium / 337 / 418 The most common ion of which element, will be smaller than the corresponding, parent atom?
All three ions are smaller than their parent atoms.
Which of the following is a noble gas? a. Ar b. N₂ c. H₂ d. O₂ e. CO₂
Ar
3. (A) Use the principles of covalent, ionic, metallic bonding and/or inter molecular forces to explain each of the following laboratory observations: - Argon has a higher boiling point than does neon
Argon has a higher boiling point than neon due to the strength of the intermolecular forces between the substance's molecules. Noble gases exhibit London dispersion forces, the weakest type of intermolecular force, which is why their boiling point is so low to begin with. London dispersion forces are caused due to the distortion of an electron cloud. Because argon has a higher atomic number than neon does, its surrounding electron cloud is bigger and causes these distortions to become bigger and stronger, hence why it has a higher boiling point.
the scientist who discovered the essential nature of acids through solution conductivity studies is
Arrhenius
Which of the following compounds has a non-zero dipole moment? a. CO₂ b. AsH₃ c. CCl₄ d. PF₅ e. SCl₆
AsH₃
What is the formula for gold (I) oxide?
Au₂O
You have 1.0 moles of each of the compounds below. Which has the greatest mass? a. Sodium Hydroxide b. Iron (III) Sulfate c. Ammonium Nitrate d. Barium Carbonate e. Lead (IV) Oxide
B ( Iron (III) Sulfate )
Which of the following elements is most similar to chlorine? a. H b. He c. Na d. Hg e. Br
Br
Which compound has bond angles of 109.5º around the central atom?
CBr₂H₂
Which of the following is nonpolar? a. IF₅ b. BrF₃ c. CF₄ d. SF₄ e. OF₂
CF₄
Which of the following molecules is the least polar? a. PH₃ b. CH₄ c. H₂O d. NO₂ e. HCl
CH₄
Which of the following should have the lowest boiling point? a. CH₄ b. C₂H₆ c. C₃H₈ d. C₄H₁₀ e. C₅H₁₂
CH₄
Which of the following substances will exhibit * only * London dispersion forces between molecules? a. H₂O b. CH₄ c. PH₃ d. CH₃OH
CH₄
Which of the following has a triple bond? a. CH₄ b. CO c. SO₂ d. NO₃⁻ e. none of these
CO
5. Answer all four of the questions below related to the properties of the alkali metal, potassium. d. The second ionization energy of potassium is greater than the second ionization energy of calcium. Explain.
Calcium has two electrons in the fourth energy level while potassium has one, so the second electron removed from potassium comes from the third energy level. This level is closer to the nucleus and its electrons are held tighter than calcium's, which means that there is more energy required to lose electrons than there is for calcium. Also, there is more electron shielding between calcium and the nucleus that potassium and the nucleus, so calcium has a lower second ionization energy.
4. Answer each of the following with respect to chemical bonding and structure c. Using Lewis Structures, explain why the ClF₃ (Chloride trifluoride) molecule is polar and the BF₃ molecule is nonpolar.
ClF₃ is polar because in the lewis structure it has two pairs of electrons on its central atom, causing it to be polar, while BF₃ does not have any pairs of electrons on its central atom making it nonpolar.
1. (A) Write the molecular equation for the following reaction: Aqueous solutions of copper(II) nitrate mixed with an aqueous solution of sodium hydroxide
Cu(NO₃)₂(aq) + 2NaOH(aq) → Cu(OH)₂(s) + 2NaNO₃(aq)
1. (B) Write the complete ionic equation for the following reaction: Aqueous solutions of copper(II) nitrate mixed with an aqueous solution of sodium hydroxide
Cu⁺²(aq) + 2NO₃⁻(aq) + 2Na⁺(aq) + 2OH⁻(aq) → Cu(OH)₂(s) + 2Na⁺(aq) + 2NO₃⁻(aq)
1. (C) Write the net ionic equation for the following reaction: Aqueous solutions of copper(II) nitrate mixed with an aqueous solution of sodium hydroxide
Cu⁺²(aq) + 2OH⁻(aq) → Cu(OH)₂(s)
Which of the following has a double bond? a. H₂O b. C₂H₂ c. C₂H₄ d. CN⁻ e. none of these
C₂H₄
What's the correct formula for the saturated hydrocarbon that contains for carbon atoms?
C₄H₁₀
What's the correct formula for the alkane that contains nine carbon atoms?
C₉H₂₀
The correct formula for iron (II) phosphide is
Fe₃P₂
The Lewis structure for which of the following contains the greatest number of lone pairs of electrons? a. CH₄ b. HF c. F₂ d. H₂O e. H₂
F₂
Which of the following species are polar? a. HBR b. NO₃⁻ c. H₂O d. SF₄ e. KrCl₄ f. I₃⁻
HBr H₂O SF₄
What is the correct formula for bromic acid?
HBrO₃ (aq)
Which of the following is named correctly? a. HCl(aq); hypochlorous acid b. (NH₄)₃PO₃; ammonium phosphate c. H₂SO₃(aq); sulfuric acid d. NH₃; ammonium ion e. HNO₃(aq); nitric acid
HNO₃(aq); nitric acid
Consider HF, NH₃, and CO₂. Which of the following statements are true? I. The electrons in each molecule tend to be attracted to the most electronegative element. II. Each molecular drawing follows the localized electron model. III. Both HF and CO₂ are linear molecules and therefore nonpolar. IV. The bond angles of NH₃ are slightly less than 109.5º because the lone pair compresses the angles between the bonding pairs.
I, II, IV (electrons in each molecule tend to be attracted to the most electronegative element; each molecular drawing follows the localized electron model; the bond angles of NH₃ are slightly less than 109.5º)
Which of the following statements is/are true? I. John Dalton provided the first expiramental support for the atom II. Ernest Rutherford proved that electrons travel in elliptical orbits around the nucleus III. J. J. Thompson proved that electrons travel in elliptical orbits around the nucelus IV. Energy in an atom is quantized, so when electrons fall to their ground state, white light can be obsereved
I. John Dalton provided the first expiramental support for the atom II. Ernest Rutherford proved that electrons travel in elliptical orbits around the nucleus
Which of the following statements are true: I. The number of protons in an element is the same for all neutral atoms of that element II. The number of electrons in an element is the same for all neutral atoms of that element III. The nuber of neutrons un an element is the same for all neutral atoms of that element
I. The number of protons in an element is the same for all neutral atoms of that element II. The number of electrons in an element is the same for all neutral atoms of that element
Which of the following has nonpolar bonds? a. I₂ b. H₂S c. OF₂ d. HF e. all are nonpolar
I₂
The first scientist to develop the theory that all atoms of a given element are identical was
John Dalton
Potassium chlorate has the formula
KClO₃
USE THIS CHART: Name / Melting point in K / First Ion. en. in KJ∙mol⁻¹ Lithium / 454 / 519 Sodium / 371 / 494 Potassium / 337 / 418 Atoms of which element have the highest second ionization energy?
Li, Since its second electron is closest to the nuclear charge.
USE THIS CHART: Name / Melting point in K / First Ion. en. in KJ∙mol⁻¹ Lithium / 454 / 519 Sodium / 371 / 494 Potassium / 337 /418 Atoms of which element have the highest electronegativity?
Li, since they are the most likely to gain electrons
What is the major attractive force in O₂?
London dispersion
magnesium reacts with bromine to form
MgBr₂
Consider the following compounds: CO, NH₃, CO₂, CH₄. H₂ Which compound has the highest boiling point?
NH₃
Which of the following molecules exhibit hydrogen bonding between their molecules? a. BH₃ b. CH₄ c. NH₃ d. C₂H₆
NH₃
You have 12.6 of an unknown substance A and 35.0 g of chlorine gas. Substance A contains 1.5 times as many molecules as the chlorine gas. What is the identity of A?
NH₃
Which of the following has an octet of electrons around the central atom? a. BF₃ b. NH₄⁺ c. PF₅ d. SF₆ e. XeF₆
NH₄⁺
Which species has the largest bond angle? a. NO₂¹⁺ b. NO₂ c. NO₂¹⁻ d. NO₃¹⁻ e. All bond angles are the same
NO₂¹⁺
Which of the following elements is an alkali metal? a. Na b. Sc c. Co d. Au e. Sr
Na
The correct name for nickel (III) phosphate is
NiPO₄
Which of the following molecules has the shortest bond length? a. N₂ b. O₂ c. Cl₂ d. Br₂ e. I₂
N₂
Which of the following bonds does not have a dipole moment? a. O-O b. B-H c. N-O d. O-H e. S-H
O-O
In which of the following is the negative end of the bond written last? a. O-S b. Br-N c. N-C d. P-Cl e. Cl-I
P-Cl
Which of the following is expected to be a polar molecule? a. PCl₄F b. BF₃ c. CO₂ d. Si(CH₃)₄ e. SCl₆
PCl₄F
The correct formula for lead (II) sulfite is
PbSO₃
Which of the following elements is an alkaline earth metal? a. Ra b. Au c. Gd d. Bi e. Cs
Ra
Titanium (IV) oxide has the formula
TiO₂
which of the following has the largest radius a. S²⁻ b. Cl⁻ c. Ar d. K⁺ e. Ca²⁺
a. S²⁻
The correct name for the aqueous solution of HC₂H₃O₂ is
acetic acid
the water solution of which of the folowing substances is the best conductor of electricity a. CO b. KCl c. C₂H₃O₂ d. CO₂
b. KCl
which compound contains both ionic and covalent bonds a. CBr₄ b. NaOH c. NaBr d. HBr
b. NaOH
which of the following is a nonmetal? a. cerium b. cesium c. carbon d. calcium e. copper
c. carbon
The correct name for an aqueous solution of H₂CO₃ is
carbonic acid
When the following equation is balencede using the smallest possible integers, what is the number in front of the substance in bold type: Al + Fe₃O₄ → Al₂O₃ + *Fe* a. 1 b. 3 c. 6 d. 9 e. 12
d. 9
Which has the least tendency to gain electrons? a. N b. Sb c. P d. Bi e. As
d. Bi
Which of the following is named INCORRECTLY? What should its name be? a. FeSO₄; iron (II) sulfate b. Sn₃(PO₄)₄; tin (IV) phosphate c. K₃P; potassium phosphide d. Fe(OH)₂; iron (III) hydroxide e. All are correct.
d. Fe(OH)₂; iron (III) hydroxide
Which of the following is a binary compound? a. O₂ b. HCN c. H₂SO₄ d. H₂S e. NaOH
d. H₂S
In which case do all three elements have similar properties because of the number or electrons in the highest energy orbital? a. Na, K, Al b. Cl, S, N c. C, Cu, Ag d. Mg, Ca, Sr e. Fe, Sn, O
d. Mg, Ca, Sr
An element's most stable ion forms an ionic compound with chlorine having the formual XCl₂. If the ion of element X has a mass of 89 and 36 electrons, what is the identity of the element, and how mnay neutrons does it have? a. Kr, 53 neutrons b. Kr, 55 neutrons c. Se, 55 neutrons d. Sr, 51 neutrons e. Rb, 52 neutrons
d. Sr, 51 neutrons
which element or ion listed below has the elctron configuration 1s²2s²2p⁶3s²3p⁶ a. S b. Ne c. Cl d. S²⁻ e. none of these
d. S²⁻
Which of the following is NOT the correct formula for the compound named? a. Hydrocyanic Acid HCN b. Calcium sulfate CaSO₄ c. Beryllium oxide BeO d. Nickel (II) peroxide Ni₂O e. Ammonium chromate (NH₄)₂CrO₄
d. nickel (II) peroxide Ni₂O
The Lewis electron dot diagrams for CO₂ and SO₂ are given. The molecular geometry and polarity of the two substances are
different because S has a greater number of electron domains (regions of electron density) surrounding it than C has.
An example of a chemical change is a. boiling alcohol b. grinding coffee beans c. digesting a pizza d. coffee spilled on a shirt e. an ice cube melting in a drink
digesting a pizza
Which of the following compounds is NOT named as an acid? a. HCl(aq) b. HCN(aq) c. H₂SO₄(aq) d. HNO₃(aq) e. NH₃(aq)
e. NH₃(aq)
an aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitate. The net ionic equation conatins which of the following species (when balanced in standard form) a. 2K⁺(aq) b. 3NO⁻₃(aq) c. 2KNO₃(aq) d. 2Na⁺(aq) e. No net ionic equation exists for this reaction
e. No net ionic equation exists for this reaction
which element or ion listed below has the electron configuration 1s²2s²2p⁶ a. Na⁺ b. Al³⁺ c. F⁻ d. Ne e. all of these
e. all of these
What is the correct name of the compound that results from the most stable ion for sulfur and the metal ion that contains 24 electrons? a. iron (II) sulfate b. iron (III) sulfide c. chromium (II) sulfide d. nickel (III) sulfate e. iron (II) sulfide
e. iron (II) sulfide
Which atomic particle determines the chemical behavior of an atom?
electron
Which of the following is the physical change? a. burning gasoline b. cooking an egg c. decomposing meat d. evaporating water e. rusting iron
evaporating water
The correct name for an aqueous solution of HCN is
hydrocyanic acid
The correct name for FeO is
iron (II) oxide
The state of matter for an object that has a definite volume but not a definite shape is
liquid
The correct name for LiCl is
lithium chloride
The fundamental unit of length in the metric system is the
meter
A cubic centimeter (cm³) is equivalent to what other metric volume unit?
milliliter
If atom X forms a diatomic molecule with itself, the bond is
nonpolar covalent
The correct name for the aqueous solution of H₃PO₄ is
phosphoric acid
Density is an example of a
physical property
VSEPR predicts that an IF₅ molecule will be which shape?
square pyramid
The name for SrCl₂ is
strontium chloride
The name for the acid H₂SO₃ is
sulfurous acid
The geometry of the SO₃ molecule is best described as
trigonal planar
In lecture, the professor named a molecule 2-ethyl-4-tertiary-butylpentane. An alert student pointed out that although the correct structure could be drawn from this name, the name did not follow systematic rules. What is the correct systematic name for the molecule?
2,2,3,5-tetramethylheptane
A student gave a molecule the following name: 2-ethyl-3-methyl-5-isopropylhexane However, her teacher pointed out that although the molecule could be drawn correctly from this name, the name violates the systematic rules. What is the correct (systematic) name of the molecule?
2,4,6,6, - tetramethylnonane
How many significant figures are in the number 1.89 x 10³?
3
a nitrogen atom needs to gain _____ electrons to achieve a noble gas configuration
3
Express 30523000 in scientific notation
3.0523 x 10⁷
You take 20.0 mL of water from a graduated cylinder and add it to the beaker of water with 15 mL. What is the new volume of water in the beaker?
35.0 mL
How many significant figures are in the number 60.02 x 10⁵?
4
C C | | C -- C -- C -- C -- C -- C -- C | | C -- C C -- C
4 - ethyl - 2,5,6 - trimethyloctane
How many of the following compounds will have Lewis structures with multiple bonds? CO, CO₂, CO₃²⁻, N₂, O₂
5
In the sum of 54.34+45.66, the number of significant figures is ...
5
The number 0.005837 expressed in scientific notation is
5.837x10⁻³
How many electrons are present in a fluorine, F, atom?
9
9.4 milliseconds is equal to how many seconds?
9.4 x 10⁻³ s
Using the rules of significant figures, calculate the following: 13.4561 - 3.48
9.98
Calculate the mass of 23.7 moles of He.
94.9
The formula for calcium hydrogen sulfate is
Ca(HSO₄)₂
USE THIS CHART: Name / Melting point in K / First Ion. en. in KJ∙mol⁻¹ Lithium / 454 / 519 Sodium / 371 / 494 Potassium / 337 / 418 From atoms of which element is it easiest to remove an electron?
K, since Coulomb's law predicts the force of attraction between the nucleus and the valence electron to be the lowest.
USE THIS CHART: Name / Melting point in K / First Ion. en. in KJ∙mol⁻¹ Lithium / 454 / 519 Sodium / 371 / 494 Potassium / 337 / 418 Atoms of which element have the largest atomic radius?
K, since it has the greatest number of occupied principal shells.
Rank the following bonds from least polar to most polar: Si-Cl P-Cl Mg-Cl S-Cl
S-Cl, P-Cl, Si-Cl, Mg-Cl
Which compound has a see-saw shape? a. CBr₂H₂ b. BH₃ c. XeCl₄ d. SF₄ e. HCl
SF₄
Which of the following bonds would be the most polar without being considered ionic? a. Mg-O b. C-O c. O-O d. Si-O e. N-O
Si-O
5. Answer all four of the questions below related to the properties of the alkali metal, potassium. c. the ionic radius of the Cl⁻ ion is greater than the ionic radius of the K⁺ ion. Explain.
The size of the chlorine ion is greater because although they have the same amount of electrons, K⁺ has a greater amount of protons giving it a greater nuclear charge than Cl⁻. The K⁺ ion will then pull its electrons closer to the nucleus and give it a smaller ionic radius.
The correct formula for titanium (IV) oxide
TiO₂
The average mass of a boron atom is 10.81. Assuming you were able to isolate only one boron atom, the chance that you would randomly et one with a mass of 10.81 is a. 0% b. 0.81% c. about 11% d. 10.81% e. greater than 50%
a. 0%
1.2 moles of oxygen atoms represent a. 0.7 x 10²⁴ atoms b. 0.4 g c. 1.0 x 10² g d. 1.9 x 10¹ atoms e. none of these
a. 0.7 x 10²⁴ atoms
The most electronegative element of those listed is a. B b. Ga c. Ti d. Al e. In
a. B
When the following equation is balenced using the smallest possible integers, what is the number in front of the substance in bold type: *Na₂S₂O₃* + I₂ → NaI + Na₂S₄O₆ a. 1 b. 2 c. 3 d. 4 e. 6
b. 2
Name the following molecule. CH₃-(CH₂)₂-CH₃
butane
When an electron in the ground state absorbs energy, it goes to a(n) ______ state.
excited
The bonds between hydrogen and oxygen in a water molecule can be characterized as
intramolecular forces
4. Answer each of the following with respect to chemical bonding and the structure of the nitrate ion, NO₂⁻, and the nitrate ion, NO₃⁻ a. Draw the Lewis structure for both the nitrite and nitrate ions
nitrate ion lewis structure
4. Answer each of the following with respect to chemical bonding and the structure of the nitrate ion, NO₂⁻, and the nitrate ion, NO₃⁻ a. Draw the Lewis structure for both the nitrite and nitrate ions
nitrite lewis structure
The correct name for HNO₂ is
nitrous acid
The binary compound PCl₃ is called
phosphorous trichloride
One of the most important characteristics of the water molecule is its_________, which allows it to surround and attract both positive and negative ions.
polarity
4. Answer each of the following with respect to chemical bonding and the structure of the nitrite ion, NO₂⁻, and the nitrate ion, NO₃⁻ b. Predict which ion (nitrite and nitrate) will have the shortest bond length. Justify your predictions.
the nitrate ion has a shorter bond length, due to resonance. the double bond moves from the one oxygen to the other. The nitrite ion has a bond order of 1.5 adn the nitrate ion had a bond order of 1.33. The larger the bond, order the shorter the bond length.
VSEPR predicts that an SbF₅ molecule will be which shape?
trigonal bipyramidal
A solution can be distinguished from a compound by its
variable composition
Which represents the greater number of atoms? a. 15.0 g S b. 15.0 g Cu c. 15.0 g Zr d. 15.0 g Sc e. all the same
a. 15.0 g S
which substance at STP conducts electricity becuase the substance contains mobile electrons a. K b. Kr c. H d. He
a. K
The name for Ba(NO₃)₂ is
barium nitrate
Consider equal mole samples of dinitrogen monoxide, aluminum nitrate, and potassium cyanide. Rank these from least to greater number of nitrogen atoms in each sample.
potassium cyanide, dinitrogen monoxide, aluminum nitrate
Consider the following compounds: CO, NH₃, CO₂, CH₄, H₂. How many of the compounds exhibit London dispersion forces?
5
Which of the following molecules are polar? a. CH₃OH b. CH₄ c. H₂O d. C₂H₆
CH₃OH H₂O
4. Answer each of the following with respect to chemical bonding and structure e. Which of the following tetrafluorides in nonpolar? Use Lewis structures to explain your conclusions. SiF₄ SF₄ XeF₄
SiF₄ and XeF₄ are both non polar because they have an even number of atoms and lone pairs of electrons hanging off of them. SiF₄ has 4 fluorine atoms hanging off of it making it balanced, and XeF₄ also has 4 fluorine atoms hanging off, but it also has two evenly distributed lone pairs of electrons hanging off, which makes it non polar. SF₄, however is polar because it only has one pair of electrons attached to the central atom, which makes it slightly negative by pushing the atoms lower and makes it polar. *draw lewis structure to show*
3. (B) Use the principles of covalent, ionic, metallic bonding and/or inter molecular forces to explain each of the following laboratory observations: - Solid silver is an excellent conductor of electricity, but solid silver iodide is not.
Silver is the best conductor of electricity because it is a metal, so it contains a higher number of movable atoms (free electrons). For a material to be a good conductor, the electricity passed through it must be able to move the electrons; the more free electrons in a metal, the greater its conductivity. Silver iodide is a poor conductor of electricity because it is polar covalent. This means that the electrons are being shared and are thus unable to move freely in contrast to silver's free electrons.
5. Answer all four of the questions below related to the properties of the alkali metal, potassium. b. the radius of the ion is smaller than the radius of the K atom. Explain.
The K⁺ ion is smaller than the parent atom, K, because metals lose electrons when they become ions to achieve the octet. This means that its electron cloud is smaller and its ionic radius is smaller than the atomic radius of K, which has more electrons. The remaining electrons of the K⁺ ion are more strongly attracted to the nucleus and are pulled closer to the center which is why it has a smaller ionic radius.
The freezing point of helium is approximately -270ºC. The freezing point of xenon is -112ºC. Both of these are in the noble gas family. Which of the following statements is supported by this data? a. Helium and xenon form highly polar molecules. b. As the molar mass of the noble gas increases, the freezing point decreases. c. The London forces between the helium molecules are *greater* than the London forces between the xenon molecules. d. The London forces between the helium molecules are *less* than the London forces between the xenon molecules. e. none of these
The London forces between the helium molecules are *less* than the London forces between the xenon molecules.
5. Answer all four of the questions below related to the properties of the alkali metal, potassium. a. the atomic radius of potassium is greater than the atomic radius of zinc. Explain.
The atomic radius of potassium is greater than that of zinc because zinc has a higher number of protons which emit stronger pulls than the protons of potassium. The electrons are attracted to the nucleus as the protons inside continue to increase in quantity. So, because of its increased number of protons zinc has a smaller atomic radius than potassium.
An atom with 40 protons has a mass number of 92. The atom is...
Zr
When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?
a *hydrogen* from one molecule and an *oxygen* from the other molecule
Which pair have approximately the same mass? a. a hydrogen and deuterium atom b. a neuron and an electron c. a proton and a neuron d. an electron and a proton
a proton and a neuron
a substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called
a strong electrolyte
Which represents the greatest mass? a. 1.0 mol Rb b. 1.0 mol Ti c. 1.0 mol Fe d. 1.0 mol Al e. all the same
a. 1.0 mol Rb
an aqueous solution of sodium sulfide is allowed to react with an aqueous solution of barium chloride. The complete ionic equation contains which of teh following species (when balenced in standard form) a. 2Na⁺(aq) b. Na⁺(aq) c. 3Ba²⁺(aq) d. 2S²⁻(aq) e. Cl⁻(aq)
a. 2Na⁺(aq)
Which of the following formulas is incorrect? a. AlO₃ b.KBr c.KNO₃ d.Li₂O e.CaSO₄
a. AlO₃
The most electronegative element of those listed is a. B b. Ga c. Tl d. Al e. In
a. B
an aqueous solution of ammonium sulfate is allowed to react with an aqueous solutoin of barium nitrate. Identify the solid in the balenced equation a. BaSO₄ b. (NH₄)₂SO₄ c. Ba(NO₃)₂ d. NH₄NO₃ e. there is no solid in the balenced equation
a. BaSO₄
which of the following compounds contains one or more covalent bonds a. CS₂ b. LiCl c. Na₂O d. CaCl₂ e. MgS
a. CS₂
an aqueous solution of ammonium carbonate is allowed to react with an aqueous solutoin of nickel(II) chloride. Identify the solid in the balenced equation a. NiCO₃ b. NH₄Cl c. NiCl₂ d. (NH₄)₂CO₃ e. there is no solid in the balenced equation
a. NiCO₃
A compound contains an unknown ion X and has the formula XCl₂. Ion X contains 20 electrons. What is the identity of X? a. Ti²⁺ b. Sc⁺ c. Ca²⁺ d. Cr²⁺ e. Mn³⁺
a. Ti²⁺
Which color of visible light has the most energy per photon? a. Violet b. Blue c. Green d. Yellow e. Red
a. Violet
Which of the following is an incorrect name for an acid? a. hydrocarbonate acid b. hydrocyanic acid c. acetic acid d. phosphoric acid e. sulfurous acid
a. hydrocarbonate acid
which metal will form a compound with the general formula X₂CO₃ when it combines with a carbonate a. lithium b. beryllium c. calcium d. aluminum
a. lithium
Which of the following statements is not true of balencing a chemical equation a. subscripts in the reactants must be conserved in the products b. coefficents are used to balence the atoms on both sides c. the law of conservation of matter must be followed e. all of the above statements are true
a. subscripts in the reactants must be conserved in the products
the electon configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶ is the correct electron configuration for the most stable form of which ion a. the strontium ion b. the calcium ion c. the krypton ion d. the barium ion e. the xenon ion
a. the strontium ion
in what type of reaction is water always a product
acid-base
The correct name for the Al³⁺ species is
aluminum ion
when a metal atom combines with a non-metal atom, the non-metal atom will a. lose electrons and decrease in size b. gain electrons and increase in size c. gain electrong and decrease in size d. lose electrons and increase in size
b. gain electrons and increase in size
the least electronegative element of those listed is a. O b. Pb c. Ba d. Cu e. Se
c. Ba
Which of the following involves a chemical change? a. boiling water b. melting ice c. chopping wood d. cooking an egg e. none of these
cooking an egg
balence the following equation in standard from and determine the sum of the coefficents: LiAlH₄(s) + AlCl₃(s) →AlH₃(s) + LiCl(s) a. 8 b. 9 c. 10 d. 11 e. 12
d. 11
when a precipitation reaction occurs, the ions that do not form the precipitate a. evaporate b. are cations only c. form a second insoluable compound in the solution d. are left dissolved in the solution e. none of these
d. are left dissolved in the solution
The correct name for P₂O₅ is
diphosphorous pentoxide
What is the major attractive force in CO?
dipole-dipole
You have two beakers on your lab table. Beaker #1 contains 32.07 g sulfur and Beaker #2 contains 74.92 g of arsenic (As). Which beaker contains the greatest number of atoms? Choose the best answer. a. Beaker #1 because one sulfur atom weighs less than one arsenic atom so you need more of the sulfur atoms to fill the beaker. b. Beaker #1 because it contains more moles of sulfur atoms than the number of moles of Arsenic atoms in beaker #2. c. Beaker #2 because arsenic has a greater mass than sulfur. d. Beaker #2 because it contains more moles of arsenic atoms than the number of moles of sulfur atoms in Beaker #1 e. Beakers #1 and #2 contain the same number of atoms because there is one mole in each.
e. Beakers #1 and #2 contain the same number of atoms because there is one mole in each.
which of the following elements is most similar to chlorine? a. H b. He c. Na d. Hg e. Br
e. Br
which of the following has the smallest radius a. S²⁻ b. Cl⁻ c. Ar d. K⁺ e. Ca²⁺
e. Ca²⁺
which of the following species would be expected to have the lowest ionization energy a. Br⁻ b. Kr c. Se²⁻ d. Sr²⁺ e. Rb⁺
e. Rb⁺
Which color of visible light has the least amount of energy per photon? a. Violet b. Blue c. Green d. Yellow e. Red
e. Red
2. A compound has a molar mass of 100 g/moland the percent composition (by mass) of 65.45% C, 5.45% H, and 29.09% O. Determine the empirical formula and the molecular formula.
empirical formula: C₃H₃O molecular formula: C₆H₆O₂
Substances whose Lewis structures must be drawn with an unpaired electron are called
free radicals
Which of the following is an SI unit for expressing the mass of a block of Au? a. m b. g c. L d. pound
g
A ________ is a summary of observed behavior, and a _________ is an explanation of behavior.
law; theory
4. Answer each of the following with respect to chemical bonding and structure d. Use Lewis structures to show why the Carbon-Oxygen bonds in the oxalate ion (C₂O₄⁻²) ion are all equal
since these is a resonace in the C₂O₄⁻² ion, all the bonds become equalized because when drawn or changed they all become the same/ interchangeable
