Passing Brenda's Class HW edition
What is the Oxidation number of each oxygen Atom in HOOH
-1
3
0.00230 has how many significant figures
5
0.054901 has how many significant figures
0.085631 ✖️1.32=0.113 in this case it's 3 sig figs.
0.085631✖️1.23 . perform operation and put into correct number of sig figs
In a sp 2- hybridized orbitals how many p- orbitals remain to for, multiple bonds
1
How many moles of H2SO4 are required to completely react with 7.20 mol of Al according to the balanced chemical reaction: 2 Al(s) + 3 H2SO4 (aq) ➡️ Al2(SO4)3 (aq) + 3 H2 (g)
7.20 mol Al ✖️( 3 mol H2SO4/ 2 mol Al) = 10.8 mol H2SO4
Solution
A homogeneous mixture is also called a
In the following Chemical reaction, which element is the reducing agent 2 Ag(s) + 2Cl- (aq) + 2N2O(l) ➡️ 2 AgCl(s) +H2(g) + 2 OH- (aq)
Ag
Gaseous mixtures
Air is an example.
Write out the Chemical formula for aluminum acetate
Al(C2H3O2)3
The products of a strong acid base reaction are
All of the above
Precision
All your shots when going mini golfing are off, but they go to the same place. Is this an example of accuracy or precision
What is the correct IUPAC name for Al2S3
Aluminum sulfide
Which element has the ground state electron configuration [Ar] 4s2 3d10 4p5
Br
(3×52.00g)+(2×(30.97g+(4×16.00g)))=345.94g
Determine the molar mass of Cr3(PO4)2.
10.0 g CO2×( 1 mol CO2 44.01 g CO2) ×(2 mol O 1 mol CO2)×(6.022×10^23 atoms O1 mol O) =2.74×10^23 atoms O
Determine the number of atoms of O in 10.0g of Co2
12 p, 10 e
Determine the number of protons and electron in Mg2+
7 protons and 10 electrons
Determine the number of protons and electrons in N3-
The intermolecular force between molecules of I2 is
Dispersion forces
3p
For which atomic orbital does n=3 and L =1
Which one of the following phases changes would be exothermic
Freezing
A human is an example of a(n)
Heterogeneous mixture
Grape juice is an example of a(n)
Homogeneous mixture
1000mL
How many milliliter are in a liter
21 p 18e
How many protons and electrons are found in a Sc3+ ion
K -F is an example of
Ionic bond
No
Is 4p7 a possible electron configuration
Concrete
NOT an example of a compound
Valance electrons in which of the following atoms experience the greatest effective nuclear charge (Zeff)
Ne
Beta particles
Negatively charged particles of radiation emitted from the decay of radioactive substances are known as
Number of electrons
Neutral atoms of isotopes of a given element have the same
Which element is the oxidizing agent CH4(g) + 2O2(g)➡️ CO2(g) + 2H2O(g)
O
Rank the following atoms in order of increasing size (smallest to largest) Li,Al, Be, Ba, O
O< Be < Li< Al < Ba
SiF₄
Of the following compounds which contains a metalloid
In a polar covalent bond ....
One atom in the bond must have higher electronegativity than the other atom
Write a chemical formula for tetraphosphorus hexasulfide
P4S6
What is the correct IUPAC name for HClO4(aq)
Perchloric acid
0.01285 - -0.00124=0.01161 5 sig figs
Perform this mathematical operation and express the answer to the correction number of significant figures: 1.285✖️10^-2 -1.24✖️10^-3
Compound
Pure substance that can be broken down into simpler substances by chemical means
8.75✖️10^5
Put the number 875000 into scientific notation
Lower,lower
Red light has a_____ frequency and a____ wavelength than ultraviolet rays
What is the noble gas core in the electron configuration for U
Rn
Which of the following phase represents sublimation
Solid ➡️ Gas
Yes objects with a density less than 1 g/cm3 will float on water. Objects with a density greater than 1 will sink.
The density of water of water is approximately 1g/cm3. Would lithium, with a density of 0.536g/cm3 will float on water?
1s2, 2s2, 2p6 3s2 3p6 4s2 3d10 4p4
The ground state electron configurations of Se atom is
7A (17)
The halogens are found in group
Which explains why the meniscus of mercury in a glass tube is convex
The lower attraction of mercury to the glass than to itself
Protons and neutrons
The nucleus of an atom contains
physical change
The process of filtration is an example of
+/- 0.001mg
The uncertainty in the measurement 13.560mg is
133
What is the mass number for an atom of xenon contains 54 protons and 79 neutrons
Marie Curie
Which scientist is credited for coining the term "radioactivity" for the spontaneous emission from atoms
N= 3, l=2 ml= -2
an Electron is shown to occupy an d orbital. Which of the following sets of quantum numbers can describe this electron
What is the correct IUPAC name for BaI2
barium iodine (II)
cooking an egg
chemical change example
594mg✖️ 1g/1000mg =0.594g
concert 594mg to g
Tearing a piece of paper
physical change example
A Liquid mixture
Definite volume and assumes the shapes of its container
Divided by
Density is defines as mass ______ volume
164.10 amu
Determine the formula weight of Ca(NO3)2
39.10amu + 79.90 amu = 119 amu
Determine the formula weight of KBr
2.11✖️10^21 atoms of As ✖️( 1 mol As➗6.022✖️10^23 atoms of As) ✖️ 74.92 g of As➗ 1 mol of As= 0.263g
Determine the mass in grams of 2.11 ✖️10^21 atoms of arsenic. The mass of one mole of arsenic is 74.92g
In a molecule of HI, what intermolecular forces are present
Dispersion and dipole dipole
What intermolecular forces are present between two molecules of CF2CF3
Dispersion only
Which of the following represent the intermolecular forces present in CO2
Dispersion only
Yes
Does 1 mole of helium, 1 mole of carbon, 1 mold of uranium all contain an equal number of atoms
Yes
Does 60Cu have the same number of neutrons as 59NI
The trend towards smaller atomic radii as one moves to the right in a periodic is
Due to the effective nuclear charge increasing
What is the shape of the 2p orbitals
Dumbbell
The energy released in the reaction F(g) + e- ➡️ F- (g) is known as the
Electron affinity
Which one of the following statements best describes electronegativity in atoms
Electronegativity is the attraction an elements nucleus has for the electrons in a chemical bond
Calcium is an example of a(n)
Element
In the same group
Elements that are most similar in their properties are found
coffee
Example of a homogeneous mixture
Silver
Example of a transition metal
Beryllium
Example of alkaline earth metal
Iron
Example of an element
Nickel
Example of an element
apple juice
Example of homogenous mixture
IR, visible, and UV
Excited hydrogen atoms emit radiation in which region(s) of the electromagnetic spectrum
5.55✖️10^11
Express the number 554,780,000,040 in scientific notation to three significant figures
Rank the following atoms in order of decreasing first ionization energies (highest to lowest) : Li,Be,Ba, F
F>Be> Li> Ba
Which term is a measure of the resistance to flow in a liquid
Viscosity
Flammability
What is a chemical property of matter
Meter
What is the name of the SI unit for length
Electron
Which particle would have the longest de Broglie wavelength traveling with the same velocity
Proton and neutron
Which particle(s) May be found in the nucleus of an atom.
Robert Millikan
Which scientist determined the charge of electron
Ernest Rutherford
Which scientist developed the nuclear model of the atom
Heisenberg
Which scientist surmised the scientific principle that the position and momentum of an electron cannot be known simultaneously with a high degree of accuracy
Proton and neutrons
Which two particles of the atom have nearly identical masses
Radio waves
Which type of electromagnetic radiation has the largest wavelength
16N
Which would be an isotope of 14 N
Schrodinger
Who developed the equation that allowed the energy of the electron to be described quantum mechanically
A more electronegative atom
Will have more attraction to the electrons in a chemical bond
A non electrolyte
Will not form any ions in aqueous solution
100g ✖️ 1cm^3/19.3g=5.18cm^3
You have a 100g sample of each metals. Find golds volume. gold d = 19.3g/cm3
+/- 0.01
You measured the mass of dry powder on a balance to be 23.76g what would you report as the uncertainty of this measurement
Convert the concentration of 0.700M Na2SO4 to g/mL
0.700 mol Na2SO4/L✖️(1L/ 1000mL) ✖️(14.04 gNa2So4 / 1molNaSO4) = 0.0994 gNa2SO4/ mL
Isotopes
28SI and 29Si are examples of
4
3.101 has how many significant figures
According to the balanced reaction below, calculate the moles of NH3 that form when 4.2 mol of N2H4 completely reacts 3 N2H4(l) ➡️ 4 NH3(g) +N2(g)
4.2 mol N2H4 ✖️ ( 4 mol NH3/ 3 molN2H4) =5.6molNH3
How many valance electrons does N have
5
The oxidation number on the phosphorus in Na3PO4 is
5
They were believed to be too noble to react with other elements
Group 18 events were called the noble gases originally because
14.5 gal✖️(3.785L/ 1gal) =54.9L
A popular car has a gas tank that holds a maximum of 14.5 gallons of fuel. What is the size of the tank in liter?
0.104km/s ✖️(0.6214mi/1km)✖️(3600s/1hr)=233mi/hr
A race car has a maxim. Speed of of 0.104 km/s. What is the this speed in miles per hours
liquid
A state of matter that has no definite shape but has a definite volume.
Gas
A state of matter with no definite shape or volume
Write out the chemical formula for phosphoric acid
H3 PO4
Write out the chemical formula for chlorous acid
HCLO2
Write out the chemical formula for chloric acid
HClO3
Which species are bronsted Lowry acids HF (aq) + NH3 (aq) ➡️ NH4+ (aq) + F- (aq) ⬅️
HF, NH4+
L
Given a particular value of the principal quantum number, which quantum number primarily determines the shape of an orbital
Solid element
Gold is an example of a
3.03✖️ 10^21 / 6.022✖️10^23 = .00503mol
How many moles of calcium do you have if you have 3.03✖️ 10^21 atoms of calcium. (The mass of one mole of calcium is 40.08g).
25.0 g C3H6 ✖️( 1 mol C3H6/ 49.09gC3H6) = 0.594 mol C3H6
How many moles of propylene (C3H6) are in 25.0 g of the substance
26
How many protons are in an atom of Fe
4
How many sig figs would this calculation have if were completed: (9.04-8.23+21.954+81.0) ✖️3.1416
5
How many significant figures does 23.070 have
Ammonium and hydrogen fluoride both have unusually high boiling points due to
Hydrogen bonding
They have equal charge
Ignoring the sign, which has a greater magnitude of change
There will be more electrons ejected
In the photoelectric effect, if the intensity of light shone on a metal increases, what will happen
Fermenting the starch
In the process of making biofuel from corn, the corn is ground, mixed with water, and then enzymes are added to ferment the starch. The fermentation produces ethanol and carbon dioxide. The ethanol is further distilled for use as a biofuel. In this process ______ is an example of chemical change
Why does the trend in noble gases boiling points increase as you go down the group
Increasing dispersion interactions
The intermolecular force found in Na+ (aq) is
Ion dipole interaction
Which periodic trend quantifies the amount of energy required to remove an electron from a neutral gaseous atoms
Ionization Energy
No
Is Fe2+ and Mn3+ Isoelectronic
No
Is this statement a part of daltons hypotheses of atomic theory: The atoms of one element are the same atoms of another element
No it is not true
Is this true about Daltons atomic theory of matter : atoms of a give. Element are identical. Atoms are indestructible
What is the correct IUPAC name for H2SO3 (aq)
Sulfurous acid
Which term is a measure of energy required to increase the surface area of a liquid
Surface tension
The charge of the electron
The Millikan oil drop experiment determined
1kg/1m3✖️1000g/1kg✖️1m/100cm✖️1m/100cm✖️1m/100cm=0.001gcm3
The Si units of density are kg/m3 but g/cm3 is more commonly used. How many g/cm3 are in 1kg/m3.
Accuracy
The accepted value of iron is 7.9 g/mL . Is 7.98g/Ml, 7.85g/ml an example of accuracy or precision.
The presence of different isotopes
The atomic mass of germanium on the periodic table is 72.630 amu. Which of the following best explains why the atomic mass is a fraction between 72 and 73
The existence of electrons
The cathode ray tube experiment determined
Hund's rule
What quantum principle stated that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having the same spin
Bohr
What scientist proposed that the electron in a hydrogen atom can only have certain energies
It is inert
What would be a chemical property of a sample of neon gas
They all have the same speed
Which color ( frequency of light travels the fastest in vacuums. Red yellow green violet or they all have the same speed
Cr
Which element has the electron configurations 1s2 2s2 2p6 3s2 3p6 4s1 3d5
B) Si
Which elements resides in the third period under group 4A (14) of the periodic table
Gamma rays
Which if the following forms of radiation has the shortest wavelengths. Red lights, microwaves, ultraviolet rays, radio waves, gamma rays
Kr
Which is the noble gas core in the electron configuration for Ru
Sr
Which of following would be chemically similar to calcium
H2O(l)➡️ H2(g) + 1/2 O2(g)
Which of the following describes a chemical change involving water
A metalloid
Which of the following does NOT describe the element Bromine
4s➡️ 3d
Which of the following electronic transitions represent an increase in energy in s multi- electron atom
S
Which of the following elements would be chemically similar to selenium
Gamma rays
Which of the following forms of radiation has the highest frequency
Pb
Which of the following is Not a metalloid
Europium
Which of the following is a lanthanide element
water
Which of the following is an example of a compound
Sc
Which of the following is not an alkali or alkaline earth element
Milli
Which of the following prefixes corresponds to 10^-3
Micro
Which of the following prefixes corresponds to 10^-6
mega
Which of the following prefixes corresponds to 10^6
Y3+
Which of the following represents a species of 39 protons and 36 electrons
S2-
Which of the following represents a species with 16 protons and 18 electrons
1s2 2s2 2p6 3s2 3p6
Which of the following represents the electron configuration of P3-
N =3, l= 1 ml =1
Which of the following sets of quantum numbers can describe a 3p electron
S2-
Which of the following species has the same number of electrons as Cl-
Fe2+
Which of the following species has the same number of protons as Fe3+
Pauli exclusion principle
Which of the following states that no two electrons can have the same set of four quantum numbers
Hypothesis
Which of the following term describes what a doctor forms when treating patients prior to ordering a medical tests
In its pure form, it is a white powder
Which of the following would be a physical property of glucose
kilo
Which of the metric prefixes corresponds to 10^3
Write a chemical formula for zinc nitrate
Zn(NO3)2
What is the condense electron configurations for Mn
[Ar] 4s2 3d5
Which of the following is the electron configuration for Ba ( condense version)
[Xe] 6s2
7.54✖️10^-8 m ✖️(10^9nm/1m)=75.4nm
Convert 7.54✖️10^-8 m to nanometers
Exact numbers
Counting 10 people in the room is a example of
H - Cl is an example of a
Covalent bond
Write the chemical formula for nitrogen trichloride
NCl3
The ejected electrons would have greater kinetic energy
Photons are shown in a piece of metal and one electron is ejected for each absorbed photon. What happens when the wavelength of light is decreased
Which of the following best describes what takes place during the solvation process
Solvent molecules surround solute molecules and pull them out into the solution
Mixture
Some liquid in a jar can be separate by physical means into two separate liquids, which can then be separated no further. The liquid is a(n):
Which hybrid orbital overlap in the C-O bond in CF2O
Sp2- sp2
Which of the following phase changes is endothermic
Sublimation
An example of a empirical formula
C7H14Cl2
Solid
Definite shape and volume
Determine the number of grams of HCL that can react with 0.750g of Al(OH)3 according to the following reaction Al(OH)3(s) + 3 HCl (aq) ➡️ AlCl3 (aq) + 3 H2O( aq)
0.750 g Al( OH)3✖️( 1mol AlCl3/ 78.00 g Al( OH)3✖️(3molHCI / 1 molAlCl3) ✖️36.46 g HCI/ 1 mol HCI = 1.05 gHCl
4
1.006✖️10^7 has how many significant figures
34.90 four sig figs
185,007➗5301
How many core electrons does an atom of beryllium contain
2
5
50.260 has how many significant figures
What is the mass percentage of C in CH3OCH3
52.14%
3
67,200 has how many significant figures
7.2✖️ 10^-3 mol hemoglobin ✖️( 6.022✖️10^23 molecules hemoglobin➗ 1 mol hemoglobin) = 4.3✖️10^21 molecules hemoglobin
A 52-kg woman has 7.2 ✖️ 10^-3 mol of hemoglobin (molar mass = 64456 g/mol) in her blood. How many hemoglobin molecules is this ?
53.0kg ✖️ (2.205lbs/1kg) =117lbs
A large stone weighs 53.0 kg. How many pounds does it weigh?
Isotopes
A mass spectrometer measures neon to have two masses: 20 and 22 atomic mass units. These are
4.8ul ✖️(1ml/1000ul)=0.0048mL
A medical laboratory test is run using an 4.8 uL blood sample. What is this volume in milliliters
Distillation
A method for separating a liquid-liquid mixture, such as water and acetone
2.70 lb ✖️(453.6g/1lb) =1220g
A person loses 2.70 lb in two weeks. How many grams did they lose.
21.3mi✖️(1.609km/ 1mi) =34.4km
An athlete preparing for a marathon runs 21.3 miles. How many kilometers did they run?
An ion
An atom has nine protons and ten electron. This makes it:
55p,78 n, 55 e
An atom of the isotope 133Cs contains how many protons neutrons and electrons
Bismuth
An example of a main group element
It's mass of 52.3g.
An example of an extensive property of copper nugget
Bar has a density of 19.2g/mL.
An example of an intensive property of a bar gold
Density
An example of physical properties of matter
(0.8900×52)+(0.0800×49)+(0.0300×50)=51.7 Amu
An unknown element X has the following isotopes 52X (84.50% abundant) 49X (8.00% abundant), 50X (7.50% abundant) what is the approximate atomic mass of X
What is the correct IUPAC name for BaHPO4
Barium hydrogen phosphate
Protons
Between electrons and protons which has the greater mass
What is the empirical formula for C₆H₁₂O₆
CH₂O
Write the chemical formula for carbon disulfide
CS2
What is the correct IUPAC name for CaBr2
Calcium Bromide
What is the correct IUPAC name for Ca(NO3)2
Calcium nitrate
Gaseous Compound
Carbon dioxide is a
Electrons
Cathode rays are composed of what fundamental particle
What is the correct IUPAC name for Cs3P
Cesium phosphide
What is the correct IUPAC name for CRBr3
Chromium(III) bromide
Which atom in the molecule CIF would have a partial positive charge
Cl
Groups
Columns on the period table are known as
What contributes to a low viscosity of liquid
Compact molecular shape
Glucose is an example
Compound
0.0134L✖️(1000mL/1L) 13.4mL
Concert 0.0134L to milliliters
Which of the following phase changes would be exothermic
Condensation
0.386g✖️(1000mg/1g) =386mg
Convert 0.386 g to milligrams.
2.3hr✖️(3600s/1hr) =8280s
Convert 2.3 hours to seconds to seconds.
2.87kg ✖️(1000g/1kg)=2870g
Convert 2.87kg to grams. Use only the metric system.
3.2ft^2 ✖️(12)^2in^2/ 1ft^2 =460in2
Convert 3.2 ft^2 to square inches
3.7cm✖️ 0.01km/ 1cm ✖️1km/1000cm =3.7✖️10^-5km
Convert 3.7cm to km
32.1 in ✖️(2.54in/1cm)=81.5cm
Convert 32.1 in to centimeters
34.0mm ✖️(1cm/ 10mm) (1in/2.54cm) =1.34in
Convert 340.0 mm to inches.
HI is an Arrhenius acid because
It proud UCD's hydronium ions in solution
What is true about vaporization
It's an endothermic process
Heterogeneous mixture
Italian dressing contains olive oil and vinegar, which will separate out from each other if left to sit. This makes the dressing a:
Write the chemical formula for potassium dichromate
K2Cr2O7
Temperature
Kelvin is the SI unit for which physical quantity
Which acid base definition classifies as acid as an electron pair acceptor
Lewis
REVIEW Lewis structures 4-1, 4-2,
Lewis structures
Wave B
Light wave A has a greater frequency than light wave B. Which has a greater wavelength
Assumes the shape of its container because it has a definite volume but no shape
Liquid
A chemical change
Magnesium metal, a gray solid, is heated in a crucible in the presence of oxygen. A white powder is collected form the crucible. This is an example of
Liquid compound
Milk is an example of a
+/- 100m
The uncertainty in the measurement 206300m is
+/-0.01mL
The uncertainty in the measurement 97.00mL is
50% they are equally abundant
There are two naturally occurring isotopes of europium, 151EU (151.0amu. And 153.0 Amu) if the atomic mass of Eu is 151.96, what is the approximate natural abundance of 151Eu?
Out of a single double and triple bond which has the shortest bond length
Triple bond
True or false: triple bonds are the strongest type of bond
True
True
True or false:two electrons can simultaneously occupy the same (n,l,ml orbital)
What happens when a ionic bond forms
Two atoms, one which is more
The phase "like dissolves like " refers to
Two molecules having the same intermolecular forces
Most of the space in an atom is empty except for am concentrated area called the nucleus
What did Rutherford's gold foil experiment determine
Total number of protons and neutrons in the atom
What does the mass number of an atom represent
Ruthenum
What element with a mass number of 100 has 56 neutrons in its nucleus
Group 6 period 5
What group and period does the element MO belong to
Energy is reduced by one half
What happens to the energy of a photon if the wavelength is doubled
Electrolysis of water to form hydrogen and oxygen gas
What is NOT an example of physical change
It's Temperature
What is a intensive property of a sample of neon gas
Sand
What is an example of heterogeneous mixture
The mass of a carbon sample
What is an extensive property of the element carbon
Individual lines of varying colors
What is observed when a noble gas is heated and the emitted light shone through a prism
37
What is the atomic number for an element whose mass number is 78 and contains 41 neutrons
114Sn
What is the atomic symbol and mass number for an atom containing 50 protons and 64 neutrons
TI
What is the atomic symbol for the element in group 4B (4) and the 4th period
Sb
What is the atomic symbol for the elements in Group 5A (15) and the 5th period
λ=531 nm× (1 m109 nm=5.31×10−7 m ν =c/λ=(3.00×10^8m/s ➗5.31×10−7 m) =5.65×1014 s−1
What is the frequency of a green light that has a wavelength of 537nm? (C= 3.00 ✖️10^8 m/s)
68
What is the mass number of zinc -68
2
What is the maximum number of electrons that can have the following set of quantum numbers: n=2 l =1 ml = 1
Hund's rule
What quantum mechanics principal states that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having the same spin
