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Science Semester 2 - Y10 > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

What is the atomic number?

A

The number of protons

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2
Q

What is the atomic mass?

A

The number of protons+neutrons

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3
Q

What are periods?

A

The rows (7)

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4
Q

What are groups?

A

The columns (18)

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5
Q

How do you determine the number of electrons?

A

In a neutral atom, the number of protons = the number of electrons

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6
Q

What does every atom want to do?

A

Wants to be stable - have all a full valence shell

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7
Q

Non-metals try to?

A

Gain electrons, become anions

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8
Q

Metals try to?

A

Lose electrons, become cations

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9
Q

Electron configuration of stable atoms (1-20)

A

2,8,8,2

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10
Q

What do the groups determine?

A

The number of valence ELECTRONS

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11
Q

What do periods determine?

A

The number of electron SHELLS

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12
Q

Periodic table trends: Atomic Radius

A

(from nucleus to valence shell) increases going down groups and decreases going left to right on a period. F is the largest, He is the smallest.

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13
Q

Periodic table trends: Metal characteristics

A

Metallic characteristics decrease as you move from left to right across the periods. This is because the atoms want to accept and gain electrons instead of lose. Increases going down to F, decreases going to He.

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14
Q

Periodic table trends: Electron Affinity

A

The amount of energy required to gain an electron. Higher electron affinity means the atom accepts the electron easier - non-metals have a higher electron affinity. Increases going up a group and going left to right across a period

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15
Q

Periodic table trends: Ionisation Energy

A

Amount of energy required to pull an electron away/lose an electron. Increases left to right on periods (because non-metals want to gain not lose) Decreases from top to bottom in groups. The further away the electrons are from the nucleus, the easier they are to remove, hence, the trend is opposite to that of the atomic radius

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16
Q

First group is?

A

Alkali metals

17
Q

Second group is?

A

Alkaline Earth metals

18
Q

3-12th groups are?

A

Transition Metals

19
Q

18th group is?

A

Nobel Gases

20
Q

Non-metals are?

A

groups 14-17

21
Q

Group 17 is?

A

Halogens (F, Cl, Br, I)

22
Q

What is ionic bonding?

A

Metal cations and Non-metal anions bond to form an ionic compound. Ionic bonding occurs when an atom gives another atoms electrons, and the overall charge of the atom is changed. This results in the two atoms bonding due to their opposite charge. It is the electrostatic attraction between oppositely charged ions. The net charge of the compound must be 0/neutral.

23
Q

Properties of ionic compounds?

A

A lot of energy is required to move ions out of their positioning, meaning they are hard to melt. At room temp they form hard brittle crystals. An example of this is Sodium Chloride (salt)

24
Q

What is covalent bonding?

A

When two non-metals bond together, they both need full valence shells to remain stable, so they share their shells. The sharing of pairs of electrons is called covalent bonding.

25
Q

What is metallic bonding?

A

Metallic bonding is the electrostatic attraction between metal ions arranged in a lattice structure with free floating electrons.

26
Q

What is metallic bonding?

A

Metallic bonding is the electrostatic attraction between metal ions arranged in a lattice structure with free floating electrons. Only the valence electrons are free to move around the atoms of the lattice.

27
Q

How is metallic bonding useful?

A

The free-floating electrons gives metals its properties such as: ductile, malleable and good conductors for heat/electricity.

28
Q

Is metallic bonding strong or weak?

A

Metallic bonding is very strong due to the high electrostatic attraction. They have very high boiling and melting points.

29
Q

How can metallic bonding make metals ductile/malleable?

A

No matter what shape the metal is, the free flowing electrons will conform to the shape, making it ductile/malleable

30
Q

Metals properties:

A

Lustrous
Good conductor
High melting point
Malleable/Ductile

31
Q

Non-Metal properties:

A

Dull
Poor conductor
Brittle

32
Q

Transition-metals properties:

A

multiple oxidation states

low reactivity
high strength
high melting/boiling points

Science Semester 2 - Y10 (3 decks)

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