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Bio 113 > Ch2 > Flashcards

Ch2 Flashcards

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Biology 101 flashcards
1
Q

Who discovered electrons?

A

J.J. Thompson in 1897

Discovered through cathode ray experiment.

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2
Q

What did R.A. Millikan determine in 1909?

A

Mass of the electron using the oil drop experiment

Mass of electron: 9.109 × 10−31 kg, Charge: e = −1.602 × 10−19 C.

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3
Q

What significant model did Earnest Rutherford propose in 1911?

A

The nucleus of the atom

Proposed through the gold foil experiment.

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4
Q

Describe Thomson’s Plum-Pudding Model.

A

Electrons are distributed throughout a positively charged sphere.

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5
Q

What was the outcome of Rutherford’s Gold Foil Experiment?

A

Disproved the plum-pudding model, leading to the nuclear atom model.

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6
Q

What does the atomic model assume about the nucleus?

A

Contains nearly all the mass of the atom and is positively charged.

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7
Q

What particles make up the nucleus of an atom?

A

Protons and neutrons.

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8
Q

What is the charge and mass of protons?

A

Charge: +1, Mass: about 1.0 u.

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9
Q

What does the atomic number (Z) represent?

A

The number of protons in an atom.

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10
Q

What is the charge and mass of electrons?

A

Charge: -1, Mass: about 1/2000 of protons.

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11
Q

What are neutrons and their role in the nucleus?

A

Neutral particles that hold protons together.

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12
Q

What is the mass number (A)?

A

The sum of protons and neutrons in an atom’s nucleus.

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13
Q

What are isotopes?

A

Atoms with identical atomic numbers but different mass numbers.

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14
Q

What defines the element in a neutral atom?

A

The number of protons equals the number of electrons.

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15
Q

Fill in the blank: The atomic number defines the _______.

A

element.

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16
Q

What is the significance of unified atomic mass units (u)?

A

Expresses masses of atoms and subatomic particles.

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17
Q

What are the categories of elements in the periodic table?

A

Metals, Nonmetals, Metalloids.

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18
Q

What is the arrangement of elements in Mendeleev’s periodic table?

A

Ordered by increasing atomic mass and similar properties.

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19
Q

What defines the modern periodic table?

A

Elements arranged by increasing atomic number.

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20
Q

What are the properties of metals?

A

Shiny, solid, conductive, malleable, ductile.

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21
Q

What is the charge of monoatomic ions in Group 1?

A

1 plus.

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22
Q

What is the charge of monoatomic ions in Group 2?

A

2 plus.

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23
Q

Identify the group and period of aluminum.

A

Group 13, Period 3.

24
Q

What is the group 16 element with the smallest atomic number?

A

Oxygen.

25
Q

What is the third-row metalloid?

A

Silicon.

26
Q

What is the fourth-row alkaline earth element?

A

Calcium.

27
Q

True or False: The mass number (A) is always greater than or equal to the atomic number (Z).

A

True.

28
Q

What do the symbols of nuclides represent?

A

Protons and neutrons in an atom’s nucleus.

29
Q

What is the average atomic mass?

A

The weighted average of masses of all isotopes of an element

It takes into account the natural abundance of each isotope.

30
Q

Which element has the lowest atomic number in its group?

A

Aluminum (Al) in group 13, row 3

31
Q

What is the only metalloid in row 3?

A

Silicon (Si) in group 14

32
Q

Where are alkaline earth metals located in the periodic table?

A

Group 2

Includes calcium (Ca) in row 4.

33
Q

How many natural isotopes does Neon have?

A

Three

34
Q

What is the mass of Neon-20?

A

19.924 u

35
Q

What is the formula for calculating average atomic mass?

A

m_Ne = (19.9924 u × 0.904838) + (20.9940 u × 0.002696) + (21.9914 u × 0.092465)

36
Q

What is the molecular mass?

A

The sum of all average atomic masses of the atoms that are chemically bonded together

37
Q

What is the formula mass used for?

A

Ionic compounds

38
Q

What is the approximate number of atoms in a copper penny?

A

27,373,000,000,000,000,000,000

39
Q

What is the mole used for?

A

To simplify a particle count

40
Q

What is Avogadro’s constant?

A

6.022 × 10^23 particles

41
Q

Fill in the blank: 1 mole is the number of atoms in exactly _______ grams of carbon-12.

A

12

42
Q

What is molar mass?

A

The mass (in grams) of one mole of a substance

43
Q

How do you convert milligrams to grams?

A

Divide by 1000

44
Q

What is the molar mass of calcium carbonate (CaCO3)?

A

100 g/mol

Estimated using whole-number values for Ca, C, and O.

45
Q

What is the number of formula units in a mole of an ionic compound?

A

Equal to Avogadro’s constant (6.022 × 10^23)

46
Q

How many moles are in 502 mg of CaCO3?

A

0.00502 mol

47
Q

How many carbon atoms are in 4.00 g of butane (C4H10)?

A

1.66 × 10^23 C atoms

48
Q

Which statement describes elements in a periodic group?

A

They have similar chemical properties.

49
Q

How many moles of carbon are in 5 moles of ethylene (C2H4)?

A

10 moles of C

50
Q

What is the value of Avogadro’s number?

A

6.022 × 10^23

Avogadro’s number is the number of atoms or molecules in one mole of a substance.

51
Q

What is the relationship between elements in a periodic group?

A

A) chemical properties.

Elements in the same group of the periodic table exhibit similar chemical properties.

52
Q

How many moles of carbon (C) are in 5 moles of ethylene (C2H4)?

A

10

Ethylene contains 2 moles of carbon per mole of ethylene.

53
Q

Which statement does not describe a physical property of chlorine?

A

A) Chlorine combines with sodium to form table salt.

This statement describes a chemical property, not a physical property.

54
Q

Which element is classified as a semimetal?

A

B) germanium

Semimetals have properties intermediate between metals and nonmetals.

55
Q

What defines isotopes?

A

An atom that has an atomic number of 34 and a mass number of 76 is an isotope of an atom that has B) an atomic number of 34 and a mass number of 80.

Isotopes have the same number of protons but different mass numbers due to varying numbers of neutrons.

56
Q

Which one of the following elements is a poor conductor of heat and electricity?

A

B) phosphorus

Phosphorus is classified as a nonmetal and is known for its poor conductivity.

Bio 113 (2 decks)

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