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Chemistry > SC2 > Flashcards

SC2 Flashcards

1
Q

Who published their ideas about atoms in 1803?

A

John Dalton.

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2
Q

What did Dalton think?

A

He thought that all matter was made of tiny particles called atoms, which he imagined as tiny solid balls.

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3
Q

What ideas did Dalton’s model include?

A
  • Atoms cannot be broken down into anything simpler.
  • The atoms of a given element are identical to each other.
  • The atoms of different elements are different from one another.
  • During chemical reactions atoms rearrange to make different substances.
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4
Q

What are the sub- particles of an atom?

A

Protons, neutrons and electrons.

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5
Q

What is the atomic number of an atom?

A

The number of protons in an atom’s nucleus.

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6
Q

What is the mass number of an atom?

A

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

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7
Q

What is an isotope?

A

When atoms of an element have the same number of protons, but different numbers of neutrons in their nuclei.

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8
Q

What do isotopes of an element have?

A
  • The same atomic number.

- Different mass numbers.

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9
Q

What is the relative atomic mass of an element?

A

The relative atomic mass of an element is the weighted average of the relative atomic masses of the isotopes in the element.

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10
Q

How do you calculate relative atomic mass?

A

Total mass of atoms divided by total number of atoms.

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11
Q

How did Mendeleev arrange the elements in the periodic table?

A

In order of increasing relative atomic mass. When he did this he noted that the chemical properties of the elements and their compounds showed a period trend. He then arranged the elements by putting those with similar properties below each other into groups. To make his classification work Mendeleev made a few changes to his order:

  • He left gaps for yet to be discovered elements.
  • He switched the order of a few elements to keep the groups consistent.
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12
Q

Why did Mendeleev leave gaps in his periodic table?

A

To place element that had not been discovered at that time. By looking at the chemical properties and physical properties of the elements next to a gap, he could also predict the properties of these undiscovered elements.

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13
Q

How is the modern periodic table arranged?

A

The elements are arranged according to their atomic number- not their relative atomic mass.

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14
Q

How are the elements arranged in the periodic table/

A
  • Rows called periods, in order of increasing atomic number.

- Vertical columns, called groups, where the elements have similar properties.

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15
Q

What side are the metal elements on in the periodic table?

A

The metals are found on the left side of the periodic table.

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16
Q

What side are the non-metal elements in the periodic table?

A

Non- metals are found on the right side of the periodic table.

17
Q

What is the electronic configuration of an atom?

A

The way in which electrons are arranged in an atom.

18
Q

What is the order of how many electrons a shell can hold?

A

2, 8, 8 and continues with 8. The first shell can only have a maximum of 2 electrons in its shell.

19
Q

How is the electronic configuration of an element related to its position in the periodic table?

A
  • The number of circles in the electronic configuration of an element is represented in the periodic table as the period number that element is situated in.
  • The number of electrons in the outermost shell of an element is represented in the periodic table as the group number that element is situated in.
  • The number of electrons in all shells of an element is represented in the periodic table as the element’s atomic number.
20
Q

How can the electronic configurations of atoms help to explain the properties of elements and the structure of the periodic table?

A

When atoms collide and react, it is the outer electrons that meet and interact. So, elements in the same group have similar chemical properties because they have the same number of electrons in their outer shell.

21
Q

What is an ion?

A

An ion is an atom or group of atoms with a positive or negative charge. Ions form when atoms lose or gain electrons to obtain a full outer shell:

  • Metal atoms lose electrons to form positively charged ions.
  • Non-metal atoms gain electrons to form negatively charged ions.
22
Q

How do metal atoms form a positive ion?

A

Metal atoms can lose electrons from their outer shell when they form ions:

  • The ions formed are positive, with more protons than electrons.
  • The ions formed have full outer shells.
23
Q

How do non-metal atoms form a negative ion?

A

The outer shell of non-metal atoms gains electrons when they form ions:

  • The ions formed are negative, because they have more electrons than protons.
  • The ions formed have full outer shells.
24
Q

How can the number of protons, neutrons and electrons be calculated in an ion?

A

By using its atomic number, mass number and ionic charge.
Remember that:
- Atomic number = protons
- Mass number = protons + neutrons
- Electrons = protons (if atom is neutral)
- Positive ions have lost electrons
- Negative ions have gained electrons.

25
Q

What is a positively charged ion called?

A

Cations.

26
Q

What is a negatively charged ion called?

A

Anions.

27
Q

How can these ions form?

A

When a metal reacts with a non-metal, by transferring electrons. The oppositely charged ions are strongly attracted to each other, forming ionic bonds,

28
Q

What are the ions in a solid ionic compound not?

A

Randomly arranged.

29
Q

What do the ions in a solid ionic compound have instead?

A

A regular, repeating arrangement called an ionic lattice.

30
Q

Why is the lattice formed?

A

The lattice is formed because the ions attract each other and form a regular pattern with oppositely charged ions next to each other.

31
Q

How is the ionic lattice held together?

A

By ionic bonds.

32
Q

What are ionic bonds?

A

Strong electrostatic forces between oppositely charged ions.

33
Q

What are ionic compounds at room temperature?

A

Solid. Melting and boiling are state changes.

34
Q

What has to be transferred to a substance in order to melt or boil it?

A

Energy.

35
Q

What is the energy needed for?

A

To break the bonds between particles in the substance:

  • Some bonds are overcome during melting.
  • All remaining bonds are overcome during boiling.
36
Q

The more energy needed…

A

The higher the melting or boiling point.

37
Q

How can a substance conduct electricity?

A

If:

  • It contains charged particles and,
  • these particles are free to move from place to place.

Chemistry (3 decks)

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