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Chemistry C4 > The Big Quiz On Atoms > Flashcards

The Big Quiz On Atoms Flashcards

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1
Q

What is an atom made of ?

A

A nucleus

Electrons

Electron shells

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2
Q

What is the atom’s nucleus made of?

A

Neutrons and protons

Positively charged - because of the proton

Nucleus take up most of the mass in an atom

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3
Q

What are electrons in an atom?

A

Move around the nucleus in electron shells

Negatively charged

Tiny

Volume (size) of the electron shells determine the size of the atom

Have no mass

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4
Q

List the properties of a proton

A

Found in the nucleus
Mass is 1
Charge is +1
Heavy

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5
Q

List the properties of a neutron

A

Heavy
No charge
Mass is 1
Found in the nucleus

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6
Q

List the properties of an electron

A

Orbit around the nucleus in electron shells

Have a mass of 0.0005
Have a charge of -1
Tiny

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7
Q

What are neutral atoms ? Why?

A

Atoms that have no charge

Number of protons are equal to the number of electrons

The charges are the same, therefore the charges cancel out and makes the atom have no charge

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8
Q

What would happen if an electron is lost in a neutral atom?

A

The atom would become an ion and be positively charged

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9
Q

What does the atomic number tell?

A

The number of protons

(It is the bottom number on a symbolic atom)

23
Na
11 < the atomic number

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10
Q

What does the mass number tell you?

A

The number of protons and neutrons

23 < mass number
Na
11

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11
Q

How do you find out the number of neutrons in an atom?

A

The atomic number

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12
Q

What does the periodic table show you?

A

The elements found so far

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13
Q

What are the vertical columns in a periodic table called ?

A

Groups

There are 8 groups in total

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14
Q

In a periodic table, how many OUTER shell electrons does “group 1” elements have ?

A

1 outer shell electron

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15
Q

In a periodic table, how many OUTER shell electrons does “group 5” elements have ?

A

5 outer shell electrons

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16
Q

What are the horizontal rows in a periodic table called?

A

Periods

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17
Q

What do the periods in a periodic table tell us about the elements?

A

How many FULL electron shells they have

Ex- period 5 elements have 5 FULL electron shells in their atom

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18
Q

If an element was in group 8 and period 4, what would it mean ?

A

The atom would have 8 electrons in its outer shell and have 4 FULL electron shells

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19
Q

What are isotopes ?

A

Different forms of the same element

Have same number of protons but different number of neutrons

20
Q

Give me an example of a pair of isotopes ?

A

Carbon-12

12
C
6

Carbon-14

14
C
6

21
Q

How many electrons is the first shell allowed to have?

A

2 electrons

22
Q

How many electrons is the 2nd electron shell aloud to have ?

A

8 electrons

23
Q

What is another word for electron shells

A

Energy levels

24
Q

What would the electron configuration for oxygen be if it has 8 protons?

A

If it had 8 protons , it must have 8 electrons

The first shell can only take up 2 electrons

2nd shell will take up 8 electrons
-after the 2 electrons went in the first shell we have got 6 electrons left (8-2)

Therefore oxygen has 2 electron shell and its electron configuration is

2,6

25
Q

What is ionic bonding ?

A

Transferring electrons where an atom loses or gains electrons to form particles

A strong bonding of 2 atoms

26
Q

Why would an atom give up an electron?

A

When they only have 1 electron in their outer shell

(Atoms always like a full outer shell)

(This will make them a positive ion as they gave up 1 electron to have a full electron shell, but they also have 1 less electron shell)

27
Q

Go an example of ionic bonding.

A

Sodium and chlorine

28
Q

How would sodium and chlorine create an ionic bond ?

A

The sodium atom will give up one of its shell (because it wanted a full outer shell) and becomes a positive atom

Chlorine (who is close to having a full shell and is 1 electron away from having a full shell) take up the thrown away atom from sodium and become a negative atom

Positive and negative atom attract each other and becomes an ionic bond

29
Q

What do ionic compounds form?

A

Giant ionic lattices

30
Q

What are ionic bonds formed by?

A

Metals and non-metals that always produce giant ionic structures

31
Q

How are ionic structures formed ?

A

Ions form a closely packed lattice arrangement.

Ions are not free to move therefore do not conduct electricity

Very strong chemical bonds between all ions

32
Q

Give me 2 examples of giant ionic structures.

A

MgO - magnesium oxide

NaCl - sodium chloride

(Both are very strong and have a high melting point due to a strong attraction between the oppositely charges ions that attach to make up the giant structure)

33
Q

What are the properties of MgO (magnesium oxide)?

A

Higher melting point that NaCl

Ions are packed together really close, strong attraction - hard to overcome

When melted , ions are free to move around - conduct electricity when melted

34
Q

What are the properties of NaCl (sodium chloride)?

A

Same as MgO but lower melting point

Can conduct electricity when dissolved in water - when dissolved, ions separate and free to move in water

35
Q

What does “a stable electronic structure” mean?

A

When atoms want a full outer shell

36
Q

What do metals do to form ions?

A

They lose electrons to become a positive ion

37
Q

What do non-metals do to become an ion?

A

They gain an electron to become a negative ion

38
Q

What happens when a metal and non-metal bond together ?

A

Make an ionic bond

39
Q

Appart from ionic bonding, what is another way atoms can join together?

A

Covalent bonding

40
Q

Explain briefly how ionic bonding works? What happens to the atoms?

A

Atoms all want a stable electronic structure (full outer shells)

Therefore they give away one (making them a positive atom) , and atoms that need an electron take one (making them a negative atom)

Positive and negative attract, therefore the 2 atoms stick together after the event.

41
Q

What is covalent bonding?

A

Sharing electrons by staying together

42
Q

Can atoms only make a covalent bond with another atom and not more atoms?

A

No

They can

They will make as much covalent bonds in order to achieve a stable electronic structure (full outer shell)

43
Q

What is a single covalent bond? Give me an example.

A

When an atom joins with another

Hydrogen gas (H2)

  • only have 1 electron
  • will join with another hydrogen
  • they only have 1 electronic shell
44
Q

What is 4 covalent bonds? Give me an example.

A

When an atom joins with 4 other atoms in order to obtain their stable electronic structure

Methane (CH4)

  • only have 4 outer electrons
  • join with 4 hydrogen to get their extra 4 electrons
45
Q

Give me 5 properties of a covalent bonds.

A

Simple molecular structure (H2O or O2)

Very strong covalent bonds

Force of attraction between each molecules are very weak - low melting and boiling point

(Force of attraction is the transparent bond that keeps all the molecules in one group) (it can easily be separated and become one individual molecule)

Do not conduct electricity - No free electrons

Chemistry C4 (6 decks)

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