Chemistry Final Review Flashcards

1
Q

What are the six steps of the scientific method?

A

Question, Background research, hypothesis, Test/Experiment, Analyze data and conclude, communicate results

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2
Q

In an experiment what is the independent variable?

A

Variable that stands alone and isn’t changed by other variables you are trying to measure.

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3
Q

What is a dependent variable?

A

What you measure in an experiment what is affected

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4
Q

What is the control variables?

A

Held constant variable, kept the same

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5
Q

Why do scientists only vary one variable in an experiment?

A

Ensures that the experimental outcomes is clearly due to one identifiable factor.

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6
Q

You want to test whether playing music in front of plants will affect their overall growth. You play constant music in front of plant 1 for a month and no music in front of plant b for a month. What would be a hypothesis for the experiment?
What is the independent, dependent, and control variables?
If at the end of a month both plants are the same height. What would be a conclusion for the experiment?

A

Hypothesis: If I play music in front of plants they will grow.

Independent: Music being played in front of plants

Dependent: growth of plants

Control: Type of plant/ light exposure

Conclusion: Playing music in front of these plants significantly causes growth

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7
Q

What is the measurement system all scientists use and why? What are examples of these?

A

SI Units because it’s easier to compare and set up on a loose 10.
Examples: Length - meter (m)
Time - second (s)
Amount of substance - mole (mol)
Temperature - kelvin (K)
Luminous intensity - candela (cd)
Mass - kilogram (kg)

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8
Q

What is the definition for accuracy and precision? What would be an example for each?

A

Accuracy: how close to a desired valve you are
Ex: if a micrometer is used to measure a 15 mm standard gauge block, and it produces a 15 mm reading, it is considered accurate
Precision: how close the results are
Ex:if you weigh a given substance five times, and get 3.2 kg each time, then your measurement is very precise.

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9
Q

How many sig figs are within 0.002030?

A

4

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10
Q

Round 306732 to 3 sig figs?

A

30700

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11
Q

What is 3.04x10^-4?

A

30400.0

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12
Q

What is 2690000?

A

2.69x10^-6

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13
Q

Give the answer in the correct number of sig figs?

A

1824> round to 1800

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14
Q

What is the definition of an element?

A

Cannot be simplified into any other substance

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15
Q

What is a compound?

A

Two or more atoms chemically bonded it definite proportions. Ex: H20, Nacl

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16
Q

What is a mixture?

A

Combo of 2 or more substances where substances maintain their properties

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17
Q

What are the four states of matter and describe each according to the space between particles and particle movement?

A

Solid, Gas, Liquid, Plasma

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18
Q

What is a solid?

A

Has definite volume and definite shape
Inter-molecular forces are strong.

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19
Q

What is a gas?

A

No definite volume and shape- weak inter-molecular forces

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20
Q

What is a liquid?

A

definite volume but no definite shape

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21
Q

What is a plasma?

A

Happens at high temps- has free floating electrons and nuclei allowing electricity to follow ex: lightning

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22
Q

What is the kinetic molecular theory? How are the particles of a liquid affected when it absorbs energy? When it release energy?

A

Explains states of matter, and is based on the idea that matter is composed of tiny particles that are always in motion. Liquid when energy is absorbed goes to a gas. When it releases it goes to a solid.

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23
Q

What phase change occurs to a liquid substance if energy is absorbed? What phase change occurs to a liquid substance if energy is released?

A

Gas

Solid

24
Q

What is happening to kinetic energy of the water during each phase of the graph and what is happening to the state of matter during each portion of the graph?

A

If energy is continually added that energy allows molecules to move faster or allow a change in state. Either releases energy or absorbs.

25
Q

When does an object sink or float in water?

A

Sink if more dense than water
Float if less dense than water

26
Q

How much mass does a 30cm3 piece of iron weigh? Density of Iron= 7.86g/cm3?

A

235.8

27
Q

What is the equation for density?

A

d=m/v

28
Q

What happens to the density of a liquid if enough energy is added? (what state would it become)?

A

Temp increases, molecules move faster and spread apart. decreases liquids density. Will become a gas.

29
Q

How are specific wavelengths of light emitted from an atom?

A

Part of an atom. Atom has a negatively charged part called electron.

30
Q

What is a proton and where is it located?

A

Positively charged particles and found in nucleus.

31
Q

What is a neutron and where is it located?

A

Neutral particles and located in nucleus

32
Q

What is a electron and where is it located?

A

Negatively charged and orbiting nucleus.

33
Q

What is the atomic number and mass number of an atom? How do you identify the atomic number and mass number of an atom?

A

Atomic #= # of protons
Mass #= Total # of protons and neutrons in nucleus

34
Q

What is a atom, ion, and Isotope?

A

Atom: smallest part of a substance that cannon be broken down chemically.

Ion: An atom or groups of atoms that has an electric charge.

Isotope: Same element different masses

35
Q

How many protons, neutrons, and electrons are within an atom of Nitrogen-14? Within Ca2+-40? Within 35 16 2 2-?

A
36
Q

How is the modern periodic table arranged and how does it differ from previous periodic tables?

A

Elements are arranged in increasing atomic number on the modern periodic table while they were arranged in atomic mass/weight in the earlier periodic table.
Sorted by number of protons, each element in the groups or columns have similar characteristics

37
Q

Where are metals, nonmetals, and metalloids located on the periodic table and what are their characteristics properties?

A

metals occupy the left three-fourths of the periodic table, while nonmetals (except for hydrogen) are clustered in the upper right-hand corner of the periodic table. The elements with properties intermediate between those of metals and nonmetals are called metalloids (or semi-metals).Sep

38
Q

What are the periodic trends as you go down the periodic table for atomic radius and ionization energy?

A

The atomic radius increases with element size (atomic number)

39
Q

What are valence electrons and why are they important?

A

The electrons in the outermost shell or energy level of an atom.

40
Q

What is an anion and cation? What are their charges? How do they become negative and positive? What types of elements form each one?

A

Cation: Ion w/a positive charge, there are more protons than e-s. The atom loses e-s

Anion: ion with negative charge, more e-s than protons. Atoms gained e-s.

41
Q

What is the Octet rule and which elements already satisfy the rule?

A

Want to get to 8 valence electrons- all atoms want their outer e level to be completely full. - 2 exceptions to Octet rule. H and He only want to 2 electrons. H will almost and always give the 1 e it has.

42
Q

What is the charge of Aluminum will become in order to be stable? Will it gain or lose how many electrons? Would it be a cation or anion?

A

+3, need to gain 5 electrons, Anion

43
Q

What is the definition for ionic bonding (electrons)? What things come together to make an ionic bond?

A

IB=m+nm
When 2 ions that are oppositely charged attract to each other.

Metals are loser and non metals are gainers`

44
Q

What is a correct formula unit? What would be the correct formula unit if Lithium and Phosphorus come together? How many electrons would be donated/received and which atom would do which?

A

Li3P, Li has 1 electron and p has 3. So p gives Li 2 electrons

45
Q

What is the correct formula for Sodium Sulfate? For Beryllium Nitride?

A

Na2(SO4)

BC3N2

46
Q

What is the correct name for Li3Po4? For CuBr2?

A

Trilithium Phosphate

Copper Bromide

47
Q

What are the properties/characteristic of ionic bond?

A

Forming crystal lattice structure, high melting and boiling points, hard, brittle

48
Q

What is the correct formula for Carbonic Acid? What is the correct name for H3P?

A

H2CO3

hydrofluoric a

49
Q

What is the definition of a covalent bond (electrons)? What things come together to make a covalent bond?

A

A chemical bond when electrons are shared between two atoms. Two electrons

50
Q

What are the properties/characteristics of polar and non polar covalent bonds?

A

polar unequal sharing of electrons, creates partial and + - charges higher melting and boiling points, non polar-equal sharing of electrons, no partial charges, lower melting and boiling points

51
Q

How can we differentiate between ionic and covalent bonds?

A

Ionic- atom donates electrons to other.
Covalent- two atom shares electrons

52
Q

What do the electrons do in a covalent bond?

A

Share electrons

53
Q

In the molecules above how many shared Paris of electrons are there between and O? How many electrons are around c? How many electrons rare being shared between c and 0? How many lone pairs are around o?

A

2 shared pairs electrons between c and 0. There are 8 electrons around c. 4 electrons being shared c and o 2 lone pairs around o.

54
Q

What is the difference between non polar covalent, polar covalent and ionic bonds?

A

If two atoms have an electronegativity difference of 0.4 or less, they form a non-polar covalent bond. If two atoms have an electronegativity difference between 0.4 and 1.8, they form a polar covalent bond. If two atoms have an electronegativity difference of more than 1.8, they form an ionic bond.

55
Q

What is the definition for polarity? What is definition for dipole?

A
56
Q
A