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ECA 1 Semester Finals > chemistry > Flashcards

chemistry Flashcards

1-8

1
Q

Define pure chemistry

A

is the pursuit of chemical knowledge for its own sake.

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2
Q

Define a theory

A

is a well-tested explanation for a broad set of observations.

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3
Q

List the three steps for solving a mathematical problem:

A
  1. analyze (determine where you are starting from), 2. calculate (if you make an effective plan, doing the calculations is usually the easiest part of the process),
  2. evanulate (after you calculate an answer you should evaluate it, find out if the answer is reasonable and if it makes sense).
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4
Q

Observations

A

when you use your senses to obtain information

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5
Q

Hypothesis

A

is a proposed explanation for an observation

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6
Q

Experiment

A

a procedure that is used to test a hypothesis

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7
Q

Which profession has benefited the most from chemistry?

A

Medicine, chemistry supplies the medicines, materials, and technology that doctors use to treat their patients.

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8
Q

Organic chemistry

A

is defined as the study of all chemicals containing carbon

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9
Q

Inorganic chemistry

A

is the study of chemicals that, in general, do not contain carbon

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10
Q

Biochemistry

A

the study of processes that take place in organisms

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11
Q

Analytical chemistry

A

is the area of study that focuses on the composition of matter

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12
Q

Physical chemistry

A

is the area that deals with the mechanism, the rate, and the energy transfer that occurs when matter undergoes a change.

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13
Q

List 3 pieces of equipment developed by alchemists which are still used today

A

beakers, flasks, tongs

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14
Q

Which important process did alchemists excel in which is vital today

A

alchemists developed the tools and techniques for working with chemicals, they designed equipment necessary.

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15
Q

Define scientific law

A

is a concise statement that summarizes the results of many observations and experiments.

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16
Q

Define a physical change

A

a change during which some properties of a material change, but the composition of the material does not change.

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17
Q

How do chemical symbols make life in chemistry better?

A

It helps show what happens to the composition of matter during a chemical change, chemists use chemical symbols to represent elements, and chemical formulas to represent compounds.

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18
Q

Mixture

A

is a physical blend of two or more components

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19
Q

Substance

A

is matter that has a uniform and definite composition

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20
Q

Homogeneous mixture

A

is a mixture in which the composition is uniform throughout.

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21
Q

Heterogeneous mixture

A

is a mixture in which the composition is not uniform throughout

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22
Q

Define an element

A

is the simplest form of matter that has a unique set of properties.

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23
Q

Define an extensive property

A

is a property that depends on the amount of matter in a sample.

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24
Q

Chemical change

A

is a change that produces matter with a different composition than the original matter.

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25
Q

Physical change

A

when some properties of a material change, but the composition of the material does not change, (can be classified a s reversible or irreversible)

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26
Q

What do subscripts in a chemical formula indicate?

A

H2O indicates that there are H+H+O

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27
Q

Accuracy

A

is a measure of how close a measurement comes to the actual or true value of whatever is measured.

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28
Q

Precision

A

is a measure of how close a series of measurements are to one another.

29
Q

What is the SI unit of measurement for length?

A

The 5 SI base units commonly used by chemists are the meter, the kilogram, the kelvin, the second, and the mole.

30
Q

Place the following prefixes into order from smallest to greatest:

A

Pico, nano, micro, milli, centi, kilo

31
Q

What is the charge and density of an atom’s nucleus like?

A

the nucleus of an atom is filled with protons and electrons, a proton is positive and an electron is negative. A neutral atom contains equal numbers of protons and electrons. The nucleus occupies most of the atom’s volume but contains little of its mass.

32
Q

Two isotopes of an element have different numbers of.._______.. And the same number of.._______

A

..neutrons and different mass numbers.. ..protons and electrons..

33
Q

All atoms of the same element have the same number of….

A

Protons but not neutrons.

34
Q

What did Rutherford’s gold foil experiment demonstrate?

A

It suggested a new theory of the atom. He proposed that the atom is mostly empty space, thus explaining the lack of deflection of most of the alpha particles. He concluded that all the positive charge and almost all the mass are concentrated in a small region that has enough positive charge to account for the great deflection of some of the alpha particles. He called this region the nucleus.

35
Q

How is the number of neutrons in an atom calculated?

A

have to subtract the number of protons from the mass number.

36
Q

Who is credited with the first idea of atoms?

A

Democritus, who came up with the idea of indivisible atoms.

37
Q

What does the mass number of an element equal?

A

The number of protons in the nucleus of the atom is equal to the atomic number. The number of electrons in a neutral atom is equal to the number of protons.

38
Q

Dalton theorized atoms are not divisible. Is this still considered true?

A

No it is false atoms are divisible are are full of smaller particles.

39
Q

The only way two electron can occupy the same orbit if they have…

A

Same energy level

40
Q

What element(s) has four electrons in its 5p sublevel

A

F, Cl, Br, I

41
Q

Stable electron configuration generally have what in their outermost level?

A

Fill putter shell two electrons

42
Q

What is the outermost configuration for the element selenium?

A

3s^2 3p^4

43
Q

Which form of electromagnetic radiation have the highest amount of energy?

A

Gamma rays

44
Q

The SI unit hertz measures…

A

Frequency

45
Q

The periodic pattern in the physical and chemical properties of elements is evident when they are placed in what order?

A

Groups

46
Q

Group A elements are collectively called…

A

Alkaline metals

47
Q

For aluminium to become an ion it must lose three electrons from what energy level?

A

P level

48
Q

Which subatomic particle plays the greatest role in determining properties?

A

Electrons

49
Q

Which period and group has the following highest electron configuration, 5s^2 5p^6

A

Group 7A and period 2

50
Q

What sublevel do the transition metals have?

A

d summer

51
Q

Which group is the alkali metals?

A

1A

52
Q

Why are the noble gases stable?

A

Filled outer shell

53
Q

List the metalloids

A

B, Si, Ge, As, Sb, Te, At

54
Q

What happens to electronegativity

A

Left to right-Increases

Down-Decreases

55
Q

Atomic size

A

Left to right-Decreases

Down- Increases

56
Q

Ionic size

A

Left to right- Decreases

Down-Increases

57
Q

All the elements in a group have the same number of…

A

Valence Electrons

58
Q

Which group has five valence electrons?

A

5A

59
Q

The ion antimonide has the same electron configuration as…

A

Xeon

60
Q

The nonmetals in Groups 5A-7A become ions by…

A

Gaining electrons

61
Q

What is the electron configuration of a chloride ion?

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6

62
Q

How many valence electrons does an ion of indium have?

A

3

63
Q

How do metals react to become more stable

A

Lose electrons

64
Q

Why do nonmetals generally gain electrons instead of losing them?

A

Because the outer shells are almost filled

65
Q

What is a molecular compound made of?

A

Molecules

66
Q

Diatomic molecule: covalent bond holds it together and how many unshared electrons pair

A 
Fluorine- single bond, 6 unshared 
Chlorine- single bond, 6 unshared
Bromine- single bond, 6 unshared
Iodine- single bond, 6 unshared
Hydrogen- single band, none
Nitrogen- triple bond, 2 unshared 
Oxygen- inadequate
67
Q

When fluorine combines with sulfur, what gas configuration will fluorine achieve?

A

Neon

68
Q

How does a covalent bond form?

A

Atoms share electrons to achieve noble gas configuration

ECA 1 Semester Finals (2 decks)

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