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1. Science 20 > A: Chemistry = Chemical Changes 1.1 The Structure of Matter > Flashcards

A: Chemistry = Chemical Changes 1.1 The Structure of Matter Flashcards

1
Q

What gives materials like aluminium, plastic, and rock salt their unique properties?

A

The elements making up these substances

Understanding the structure of the atom is essential to answer this.

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2
Q

What are the three major particles that make up an atom?

A

Protons, neutrons, and electrons

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3
Q

Define a proton.

A

A positively charged particle located in the nucleus of an atom

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4
Q

Define a neutron.

A

A neutral particle located in the nucleus of an atom

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5
Q

Define an element.

A

A pure substance that cannot be broken down into simpler substances by chemical means

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6
Q

What is an atom?

A

The smallest part of an element that has all the properties of that element

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7
Q

Fill in the blank: An atom consists of a nucleus containing ______ and ______.

A

Protons and neutrons

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8
Q

True or False: The electron cloud surrounds the nucleus of an atom.

A

True

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9
Q

What is the atomic number?

A

The number of protons in the nucleus of an atom

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10
Q

What is the atomic mass?

A

The average mass of the atoms of an element including all isotopes

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11
Q

What is the mass number?

A

The total number of protons and neutrons in an atom

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12
Q

How do you determine the average number of neutrons in an atom?

A

Subtract the number of protons (atomic number) from the atomic mass and round to the nearest whole number

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13
Q

What is the relationship between protons, neutrons, and the mass number?

A

The sum of the number of neutrons and protons is called mass number

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14
Q

What is a hydrogen atom’s atomic number?

A

1

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15
Q

What is a carbon atom’s atomic number?

A

6

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16
Q

True or False: Protons and neutrons occupy volume in an atom.

A

False

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17
Q

Where are protons and neutrons located in an atom?

A

In the nucleus

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18
Q

What occupies the larger region surrounding the nucleus of an atom?

A

Electrons

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19
Q

Fill in the blank: The space outside the nucleus is often described as ‘an ________ cloud.’

A

electron

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20
Q

What makes the atom of one element differ from the atoms of all other elements?

A

The number of protons

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21
Q

What is the significance of the mass number?

A

It is always a whole number

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22
Q

What is the average number of neutrons in the most common form of an atom?

A

The difference between the atomic number and the mass number

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23
Q

True or False: Electrons have more mass than protons and neutrons.

A

False

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24
Q

What particles make up most of the atom’s mass?

A

Protons and neutrons

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25
Q

What explains why one atom will bond with another?

A

The electrical characteristics of protons and electrons.

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26
Q

What happens when two atoms approach one another?

A

They may initially repel due to interactions between negatively charged outer electrons.

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27
Q

What exerts greater attractive forces on electrons in the vicinity of an atom?

A

The large concentration of positive charge in each nucleus.

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28
Q

Why are fast-moving electrons bound to the nucleus?

A

Because oppositely charged objects are attracted to each other.

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29
Q

In a neutral atom, what is equal?

A

The number of protons and electrons.

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30
Q

What are protons and neutrons made up of?

A

Even smaller particles called quarks.

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31
Q

What determines how an atom bonds with other atoms?

A

The protons, neutrons, and electrons that make up each atom.

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32
Q

What do the particles of an atom determine?

A

The physical and chemical properties of each substance.

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33
Q

What questions should you ask to understand the properties of a material?

A

• What is the structure of the atoms within that substance?
• How are the protons, neutrons, and electrons interacting within that substance?

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34
Q

What insights can you gain from understanding the properties of atoms in a substance?

A

Information about the unique properties of a substance and how the atoms within it interact.

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35
Q

What is the name of the diagram commonly used to represent atoms?

A

Bohr diagram

Named after the scientist Niels Bohr.

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36
Q

Who developed the idea of energy levels in atoms?

A

Niels Bohr

Niels Bohr is a physicist known for his contributions to understanding atomic structure.

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37
Q

What determines the number of electrons that can occupy an energy level?

A

The energy level itself

Only a certain number of electrons can occupy each specific energy level.

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38
Q

Where do electrons with the lowest energy reside in relation to the nucleus?

A

In the energy levels closest to the nucleus

Electrons in these levels are at a lower energy state.

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39
Q

Fill in the blank: An _______ is a specific region surrounding the nucleus that is available for electrons.

A

energy level

Energy levels are crucial for understanding atomic structure.

40
Q

True or False: Electrons in higher energy levels have less energy than those in lower energy levels.

A

False

Electrons in higher energy levels have more energy.

41
Q

Who developed the idea of energy levels in atoms?

A

Niels Bohr

Niels Bohr is a physicist known for his contributions to understanding atomic structure.

42
Q

What determines the number of electrons that can occupy an energy level?

A

The energy level itself

Only a certain number of electrons can occupy each specific energy level.

43
Q

Where do electrons with the lowest energy reside in relation to the nucleus?

A

In the energy levels closest to the nucleus

Electrons in these levels are at a lower energy state.

44
Q

What is the order in which energy levels are filled?

A

Energy levels closest to the nucleus are filled first, followed by energy levels farther from the nucleus.

45
Q

What do Lewis dot diagrams represent?

A

A representation of an atom that shows only the valence electrons

Chemists focus on these outermost electrons for chemical interactions.

46
Q

What is the first step in drawing a Lewis dot diagram?

A

Write the chemical symbol

This symbol represents the inner electrons and the nucleus.

47
Q

What should be determined in the second step of creating a Lewis dot diagram?

A

The number of electrons in the outermost energy level

This information is crucial for accurately representing the atom.

48
Q

In a Lewis dot diagram, how are the outer energy level electrons represented?

A

Using dots

Each dot represents one electron in the outer energy level.

49
Q

Where can dots be placed in a Lewis dot diagram?

A

North, east, south, or west sides of the symbol

Each position can hold a maximum of two electrons.

50
Q

When should electrons be doubled up in a Lewis dot diagram?

A

Only after all other positions contain at least one electron

This ensures proper representation of electron distribution.

51
Q

What is the first vertical column of the periodic table called?

A

Alkali metals

Alkali metals are known for being very reactive.

52
Q

What do elements in the first vertical column of the periodic table have in common?

A

Very similar properties such as being highly reactive

This similarity is due to their group classification.

53
Q

Which group of elements is located in the second-last column on the periodic table?

A

Halogens

Halogens are also very reactive.

54
Q

What is the last group on the right side of the periodic table called?

A

Noble gases

Noble gases are characterized by their lack of reactivity.

55
Q

What is unique about noble gases compared to alkali metals and halogens?

A

Not reactive

Noble gases have very low reactivity due to their full electron shells.

56
Q

What is unique about noble gases compared to alkali metals and halogens?

A

Not reactive

Noble gases have very low reactivity due to their full electron shells.

57
Q

What happens when two atoms come into close proximity to one another?

A

Their electrons are attracted to both nuclei.

58
Q

What do the nuclei of two approaching atoms do?

A

Each nucleus begins to attract the electrons of the other atom.

59
Q

What are the electrons involved in atomic bonding called?

A

Valence electrons.

60
Q

Valence electrons are defined as _______.

A

[those that are in the outer energy level of an atom]

61
Q

What is the significance of full outer energy levels in atoms?

A

Stable atoms rarely form bonds due to their filled outer energy levels.

This characteristic is observed in noble gases.

62
Q

Name the noble gases.

A
  • Helium
  • Neon
  • Argon
  • Krypton
  • Xenon
  • Radon

These gases have full outer energy levels.

63
Q

How do the arrangement of protons, neutrons, and electrons affect an atom?

A

The arrangement determines the properties of an atom.

This includes stability and reactivity.

64
Q

What are the three ways atoms can obtain a noble gas configuration?

A
  • Gaining electrons
  • Losing electrons
  • Sharing electrons

These processes help atoms achieve filled outer energy levels.

65
Q

True or False: Noble gases are reactive due to their filled outer energy levels.

A

False

Noble gases are stable and rarely react.

66
Q

Fill in the blank: Atoms can become more like a noble gas by _______.

A

[gaining or losing or sharing electrons]

67
Q

What happens to an atom when it gains electrons?

A

It fills empty spaces in its outermost energy level.

It also becomes negatively charged.

68
Q

What is the notation for gaining one electron?

A

+ 1e

69
Q

What is the atomic number of chlorine?

A

17

70
Q

How many electrons does a chloride ion have?

A

18

71
Q

What is the charge of a chloride ion?

A

-1

72
Q

What results from an atom having more electrons than protons?

A

The net charge changes to a negative charge.

73
Q

What is a charged atom called?

A

An ion.

74
Q

True or False: Non-metallic atoms tend to become positively charged ions.

A

False.

75
Q

Fill in the blank: A charged atom or group of atoms is called a/an _______.

A

ion

76
Q

What is an atom or group of atoms that has an overall positive charge?

A

Cation

A cation is formed when an atom loses electrons.

77
Q

What is a negatively charged ion called?

A

Anion

Anions are formed when an atom gains electrons.

78
Q

What happens to an atom when it loses electrons?

A

It becomes positively charged

The atom has fewer electrons than protons after losing electrons.

79
Q

What is the charge of a sodium ion after losing one electron?

A

1+

Sodium (Na) has 11 protons and 10 electrons after losing one electron.

80
Q

What is the electron configuration of a sodium atom?

A

1s² 2s² 2p⁶ 3s¹

Sodium has one electron in its outermost energy level.

81
Q

Which type of atoms have a tendency to form cations?

A

Metallic atoms

Metallic atoms typically lose electrons to achieve a stable electron configuration.

82
Q

True or False: An atom becomes a cation by gaining electrons.

A

False

A cation is formed by the loss of electrons, not by gaining them.

83
Q

What happens to an atom when it loses electrons?

A

It becomes positively charged

The atom has fewer electrons than protons after losing electrons.

84
Q

True or False: An atom becomes a cation by gaining electrons.

A

False

A cation is formed by the loss of electrons, not by gaining them.

85
Q

What is a covalent bond?

A

A covalent bond is formed when an atom shares electrons with other atoms.

86
Q

Which types of atoms typically form covalent bonds?

A

Non-metallic atoms.

87
Q

What do atoms achieve by sharing electrons in a covalent bond?

A

Atoms complete their outer energy levels.

88
Q

Fill in the blank: An atom can share electrons with other atoms to produce a _______.

A

[covalent bond]

89
Q

True or False: Covalent bonds are formed only between metallic atoms.

A

False

90
Q

What is the smallest part of each element that still has the properties of that element?

A

An atom

Atoms are the fundamental building blocks of matter, representing the basic unit of a chemical element.

91
Q

How are all atoms of an element, like hydrogen, characterized?

A

They are identical

Each element has unique atoms that are distinct from those of other elements.

92
Q

What basic parts make up atoms of different elements?

A
  • Protons
  • Neutrons
  • Electrons

These subatomic particles are common to all atoms, regardless of the element.

93
Q

What do vertical columns on the periodic table represent?

A

Groups or families

Elements in the same group have the same number of valence electrons.

94
Q

What do elements in the same group or family on the periodic table have in common?

A

The same number of valence electrons and similar properties

This similarity affects their chemical behavior and reactivity.

95
Q

When is an atom most stable?

A

When its outer energy level is filled with electrons

Stability is often achieved through gaining, losing, or sharing electrons.

96
Q

What can atoms do to achieve a full outer energy level?

A
  • Gain electrons
  • Lose electrons
  • Share electrons

These processes lead to the formation of chemical bonds.

1. Science 20 (52 decks)

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