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Biology 1 > Unit 1 (Chapter 2, Part 1) > Flashcards

Unit 1 (Chapter 2, Part 1) Flashcards

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1
Q

What is the study of the nature of atoms and molecules, with the exception of those that contain rings or chains of carbon?

A

Inorganic Chemistry

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2
Q

What is Organic Chemistry?

A

The study of carbon-containing molecules.

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3
Q

What is anything that has mass and takes up space?

A

Matter

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4
Q

What are the three states of matter in living things?

A

Solid, liquid, or gas.

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5
Q

What do atoms consist of?

A

Subatomic particles (Physicists like to uncover their properties)

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6
Q

What is the simplest atom and is roughly one-millionth the diameter of human hair?

A

Hydrogen

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7
Q

Specific types of atoms, like nitrogen, hydrogen, oxygen and others, is called a(n) ________ which is defined as a pure substance made of only one kind of atom?

A

Element

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8
Q

What are the (3) subatomic particles found within atoms?

A
  1. Protons +
  2. Neutrons 0
  3. Electrons -
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9
Q

What is a positively charges particle found in the nucleus of an atom?

A

Proton

The number of protons in an atom is called the atomic number and defines each type of element.

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10
Q

What is the neutral particle found in the nucleus of an atom?

A

Neutron

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11
Q

What is a negatively charged particle found in orbitals around an atomic nucleus?

A

Electron

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12
Q

What is an atomic nucleus and what does it contain?

A

It is the center of an atom and contains protons and neutrons.

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13
Q

T/F All atoms have the same number of protons and electrons.

A

True

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14
Q

T/F Like charges repel each other while opposite charges attract each other.

A

True

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15
Q

Bonus: What is a simple hydrogen atom made up of? What about a helium atom?

A

Hydrogen: 1 Proton and 1 Electron

Helium: 2 Protons, 2 Neutrons, and 2 Electrons

Substracting the 2 electrons in a Helium atom, and you get positively-charged alpha particles.

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16
Q

Why does an entire atom have no net electric charge?

A

Because the number of negatively charged subatomic particles match the number of positive charged subatomic particles within the nucleus.

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17
Q

In 1901-1911, Ernest Rutherford discovered what about the atom and how did he do it?

A

He knew atoms contained charged particles and hypothesized that they were distributed evenly within the atom.

He shot alpha particles at thin gold foil and found that 98% of them were not refracted or deflected meaning that volume of a atom is empty space.

Today, we know that more than 99.99% of an atom’s volume is outside the nucleus. The nucleus accounts for only about 1/10,000 of an atom’s diameter. Most of the atom is empty space!

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18
Q

What did scientists envision the structure of an atom before Rutherford’s experiment?

A

Scientists were aware that atoms contained charged particles. Many believed that the positive charges and mass were evenly distributed throughout the atom; diffuse.

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19
Q

T/F It is possible to detect the exact location of an electron.

A

False.

We can only describe the region of space surrounding the atomic nucleus in which there is a high probability of finding that electron.

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20
Q

What is the region surrounding the nucleus of an atom where the probability is high of finding a particular electron?

A

Orbital

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21
Q

What is the difference between s orbitals and p orbitals?

A

S orbitals are spherical and p orbitals are similar to a propeller or dumbbell.

There are many more different kinds of orbitals as electrons gain more energy.

22
Q

What is the maximum number of electrons an orbital can contain?

A

2

23
Q

What is the region around an atom’s nucleus where electrons reside where larger atoms have more and smaller atoms have less?

A

Electron Shell

24
Q

Bonus: How many electron shells does the heaviest elements contain?

A

7

25
Q

What is energy defined as?

A

The ability to promote change or do work.

26
Q

What type of energy does electrons have?

A

Kinetic energy; the energy of moving matter.

27
Q

How are electron shells numbered?

A

The closest shell to the nucleus is 1.

28
Q

Which shell within ALL atoms has room for only two electrons, which spin in opposite directions within a spherical s orbital (1s)?

A

The innermost electron shell or shell 1.

29
Q

How many orbitals does the second electron shell of an atom hold?

A

One spherical s orbital (2s) and three dumbbell-shaped p orbitals (2p).

Therefore, the second shell, can hold up to four pairs of electrons, or 8 in total. Also, s orbitals have less energy than the p orbitals so they fill up first, one electron at a time.

30
Q

Which electron shell holds the lowest energy electrons in an atom and fills up first?

A

1s. In subsequent shells, the first orbital with the lowest energy is always spherical and has room for only two electrons.

31
Q

What is the difference between an electron shell and an orbital?

A

An electron shell is a region outside the nucleus of an atom occupied by electrons of a given energy level. More than one orbital can be found within an electron shell. An orbital may be spherical or dumbbell-shaped and contains up to two electrons.

32
Q

What do atoms with unfilled outer electron shells typically tend to do?

A

They tend to share, release, or obtain electrons to fill their outer shells.

33
Q

What is the name of an electron in the outermost shell of an atom that is available to share with other atoms?

A

Valence electrons. Such electrons allow atoms to form chemical bonds with each other.

When a chemical bond is formed with two or more atoms, they create a new substance called a compound.

34
Q

With the exception of ions, what is the net electrical charge of an atom and why?

A

The net electrical charge of an atom is zero because atoms have the same number of positively charged protons and negatively charged electrons.

35
Q

How the elements organized chronologically. horizontally and vertically in the table of elements?

A

Chronologically, elements are in order of their atomic number which is the number of protons in the nucleus.

Elements are organized horizontally by the number of electrons in their outer shells and further so by the amount of electron shells.

Ex. Hydrogen is #1 because it has 1 proton and 1 electron shell. Sodium is #11 because it has 11 protons and it is on the 3rd row because it has 3 electron shells.

Elements are organized vertically by how many shells they have chronologically. Ex. Row 1 = 1 electron shell
Row 2 = 2 electron shells and so on.

36
Q

What are the rows called in the Table of Elements?

A

Periods

37
Q

What are the columns called in the Table of Elements?

A

Groups

38
Q

What is significant about how elements are GROUPED in the Table of Elements?

A

The similarities within a group occur because they have the same number of valence electrons, and therefore, they have similar chemical bonding properties.

39
Q

Out of the three subatomic particles, what are virtually equal mass? Protons, neutrons, and electrons.

A

Protons and neutrons.

40
Q

How much more mass does protons and neutrons have compared to electrons?

A

1,800+ times more mass… so the mass of the electrons is ignored in calculating the atomic mass.

41
Q

What is an atom’s mass relative to the mass of other atoms?

A

Atomic Mass (Hence, the hydrogen atom, the simplest of the elements, who mass is 1.008 because of the 1 proton and 1 electron (ignored))

By convention, the most common form of carbon, which has six protons and six neutrons, is assigned an atomic mass of exactly 12).

42
Q

BONUS: What is the mass of a proton and a neutron RELATIVE to an electron?

A

Proton: 1836 times the size of an electron
Neutron: 1839 times the size of an electron

43
Q

What is the difference between weight and mass?

A

Weight is derived from the gravitational pull on a given mass, while mass is a measurement of space the subject takes up in a vacuum.

44
Q

What is atomic mass measured in?

A

Daltons (Da), equal to the atomic mass (amu)

After John Dalton, who postulated that matter is composed of tiny indivisible units called atoms and laid the groundwork for atomic theory.

45
Q

What is another name for Daltons?

A

Atomic Mass Units (amu)

The unified atomic mass unit, a more modern abbreviation, is just a u.

Remember: The average atomic mass on the periodic table of elements is the AVERAGE of all isotopes of a given element not just one kind of the element. There are many different versions of an element (same amount of protons but differing amounts of neutrons) and their significance in our environment.

46
Q

What is 1 amu equal to? And really is a benchmark for atomic mass measurements.

A

1/12 the mass of a carbon atom or about the mass of a proton or hydrogen atom.

Remember: the mass of an electron is ignored since they are over 1800+ times smaller than a proton or neutron. A hydrogen atom has 1 proton and 1 neutron.

47
Q

T/F 1 g of carbon contains more atoms than 1 g of hydrogen.

A

False.

Because Hydrogen is a smaller atom, 1 g of carbon would actually have less atoms since it is a bigger atom.

48
Q

What is a mole (mol)?

A

The amount of any substance that contains the same number of particles as there are particles in exactly 12 g of carbon.

49
Q

What is Avogadro’s number?

A

6.022 x 10^23 (number of atoms)

1 mole of any element contains the same number of atoms (6.022 x 10^23)

50
Q

Why do we use moles in chemistry?

A

Because in chemistry we will not deal with a single atom, it is salient that we convert average atomic mass to the masses of samples (samples you would see in a lab)

Biology 1 (37 decks)

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