Chem 6A Fund. A-M Chapter 1-5

Front 1

What is physical property? What are the characteristics?

Back 1

Characteristic we can observe or measure without changing identity of the substance; i.e. Hardness, boiling points, color, state of matter, density, freezing points.

Front 2

What is chemical property?

Back 2

ability of a substance to change into another substance.

Front 3

what is intensive property? What is an example.

Back 3

property that is independent of the mass of the sample. i.e. density

Front 4

What is extensive property? What is an example.

Back 4

Property that does not depend on the mass "extent" of the sample. i.e. volume

Front 5

Categorize the following properties of Uranium as physical or chemical?
1. Ur melts at 1135 degrees c
2. Ur is a solid @ room temp.
3. Acid reacts w/ Ur

Back 5

1. Physical
2. Physical
3. Chemical

Front 6

Which of the following represent a set of isotopes?
1. 20 p and 20 n
2. 21 p and 19 n
3. 18 p and 22 n
4. 19 p and 22 n
5. 21 p and 20 n

Back 6

pair 2 and 5 because an isotope has the same number of protons but different number of neutrons.

Front 7

true or false the energy of an atom is increased when electromagnetic radiation is emitted from it.

Back 7

false: the energy of an atom is decreased.

Front 8

What do groups in a periodic table have in common?

Back 8

similar properties

Front 9

What do periods in a periodic table have in common?

Back 9

Similar valence shell electrons.

Front 10

Which of the following is the least reactive?
1. Na
2. K
3. Li
4. Cs

Back 10

Li because the elements are more reactive as you go down a group

Front 11

Calculate the kinetic energy of our chemistry book that weights 1.50 kg just before it hits the floor if it is traveling at 4.4 m/s

Back 11

Ekinetic=1/2(m)(v)^2
answer: 14 j

Front 12

How many molecules are in 1.058 moles of h20?

Back 12

1.058x(6.02214x10^23)=
6.371x10^23 molecules.

Front 13

Find the mass of a sulfur atom and the number of atoms in a 1 gram sample of the element.

Back 13

you do mass divided by avogadros number and you get 5.324x10^-23 g/atom and just convert to grams since there is only one atom the answer would be 5.324x10^-23 grams for the mass of a sulfur atom then do 1 g over the mass of the sulfur atom which would give you 1.878x10^22 atoms in 1 gram of a sulfur atom.

Front 14

How many atoms are in 3.000 moles of water?

Back 14

3.000 moles times avogadros number times 3 atoms which equals 5.420x10^23atoms.

Front 15

What is the unit of frequency?

Back 15

s^-1 or Hz

Front 16

true or false long wavelengths lead to small frequencies and short wavelengths lead to high frequencies.

Back 16

TRUE.

Front 17

Calculate the wavelength of a red light that has a frequency of 4.27x10^4 Hz in nanometers

Back 17

c is a constant=2.998x10^8 m/s
so in the equation c equals wavelength times frequency. to solve for wavelength it would be the constant over the frequency. therefore the answer is 702 nm.

Front 18

If the energy for red light is 2.83x10^-19 J/photon then what would the energy be for 1.00 mol of photons of light.

Back 18

convert photons to moles using avogadros number then multiply by mol then convert to kj. answer should be 172 kj

Front 19

Calculate the wavelength of a particle of mass 1g traveling at 1 m.s^-1

Back 19

based on wavelength duality equation wavelength equals plancks constant over mass times speed the answer is 7x10^-3 remember that your mass must always be in kg unless asked.

Front 20

What is the equation to solve for the energy of a photon.

Back 20

plancks constant times frequency.

Front 21

If an electron is confined to a one-dimensional box 200 pm in length, calculate the zero-point energy. use the equation E=n^2h^2/8mL^2

Back 21

answer:1.51x10^-18 J

Front 22

Arrange antimony, bismuth, and phosphorus in order of decreasing atomic radius.

Back 22

Bi>Sb>P

Front 23

What is orientation in space that an atomic orbital is associated with.
n,l,ml, or ms

Back 23

the magnetic quantum number ml

Front 24

What is shape that an atomic orbital is associated with.
n,l,ml, or ms

Back 24

the angular momentum quantum number l

Front 25

What is size that an atomic orbital is associated with.
n,l,ml, or ms

Back 25

the principal quantum number n

Front 26

in a single atom how many possible orbitals have the principal quantum number n=4

Back 26

16

Front 27

which of the following would be most REACTIVE with air and water?
1.Ba
2. Mg
3. Ga
4. Br
5. They are equal in reactivity

Back 27

Ba because it is the farthest down remember at the bottom of each group is the most reactive.

Front 28

TRUE or FALSE The energy of electromagnetic radiation increases as its frequency increases.

Back 28

TRUESIESSS

Front 29

TRUE or FALSE this arrangement is in order of decreasing size.
S^2->Cl^->K^+>Ca^2+>Ga^3+

Back 29

TRUESIESSSS.

Front 30

one molecule of a compound weighs 2.03x10^-22g the compound is:
1.PdO
2.Al2O3
3,SiO4
4.SO
5. none of these

Back 30

PdO just divide the molar mass by the avogadros number.

Front 31

Give the three quantum number of hyrdogen.
n=
l=
ml=

Back 31

n=1
l=0
ml=0

Front 32

how many planar nodes does a d orbital have?

Back 32

2

Front 33

True or false atomic radius generally increase from left to right across a period and decreases down a group.

Back 33

FALSE. atomic radius generally decrease from left to right across a period and increases down a group.

Front 34

True or false ionic radii generally increases down a group and decrease from left to right across a period.

Back 34

TRUE TRUE

Front 35

state whether it is an ionization energy equation or electron affinity equation:
1. X(g) +e-(g)->X-(g)
2. X(g)->X+(g)+e-(g)

Back 35

1. electron affinity
2. ionization energy

Front 36

ionization _____down a group and left to right it ______.

Back 36

decreases, increases

Front 37

what is an atom when it loses valence electrons?

Back 37

cations

Front 38

What is an atom when it gains valence electrons?

Back 38

anions

Front 39

what is the ground state electron config for bromine?

Back 39

[Ar]3d10 4s2 4p5

Front 40

what is electron config for Fe2+ ion

Back 40

[Ar] 3d6

Front 41

what is the name of P4Se3

Back 41

tetraphosphorus triselenide

Front 42

what is Fe2O3

Back 42

Iron(III) oxide

Front 43

In naming acids match each of the following to what it should be changed to (it can be used more than once:
1.-ite A.-ic
2.-ide B.eous
3.-ate

Back 43

1.b
2.a
3.a

Front 44

a compound containing B and H contains 81.10% of B what is the empirical formula?

Back 44

100-81.10=18.9%H convert B and H into moles and divide by the lowest number of moles and you should get B2H5

Front 45

if 0.5 mol of a tin compound weighs 313g what is the molecular formula?
1.Sn2I8
2.SnI4
3.Sn4I16

Back 45

2. SnI4 because its molecular weight is 626 g/mol sam as 0.5mol/313g

Front 46

True or false concentration tells us how much solute is dissolved in the solvent. whether is it true or false provide us with the equation.

Back 46

TRUE. M=n/v

Front 47

What mass of oxalic acid H2C2O4 is required to make 250 mL of a 0.05 M solution?

Back 47

n=Mv you should get 1.13 g H2C2O4

Front 48

You have 50.0 mL of a 3.0 M NaOH what volume is needed to get 0.50 M of NaOH

Back 48

M1V1=M2V2
you should get .30 L

Front 49

Acetic acid CH3COOH can be purchased as "glacial acetic acid" which is %100 CH3COOH has a density of 1.05g/mL calculate molarity of "glacial acetic acid"
1)0.175M
2)17.5 M
3)1.05 M
4) 0.0105M
5)100 M

Back 49

get it?! 17.5 M HAHAHAHAH