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Grade 9 2nd Periodic Test > Science > Flashcards

Science Flashcards

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Periodic Table flashcards
1
Q

These are called the building blocks of matter.

A

Atoms

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2
Q

What is the most widely accepted model of the atom?

A

Niels Bohr’s planetary model.

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3
Q

What are the three main types of elements?

A

Metals, Metalloids, and Non-Metals.

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4
Q

How many valence electrons is the maximum amount an element can have?

A

8

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5
Q

How do you determine the number of valence electrons an element can have?

A

The number of valence electrons of an element can be seen by counting the group number of the element in the periodic table from left to right. (Excluding transition metals)

(Also except helium, which has 2 valence electrons.)

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6
Q

The atomic number of an element is the same amount as the number of protons and electrons it has. (Unless it’s an ion) True or False?

A

True

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7
Q

These are the electrons on the outermost energy level of an atom.

A

Valence Electrons

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8
Q

Atoms gain, lose, and share electrons to gain 8 valence electrons. What rule is this?

A

The Octet Rule

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9
Q

Non-metals lose valence electrons. True or False?

A

False. They usually gain/receive electrons.

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10
Q

Metals lose/give valence electrons. True or False?

A

True

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11
Q

What do atoms become when they give/receive electrons?

A

Ions

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12
Q

What is a pawsitively charged ion?

A

Cation

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13
Q

What is a negatively charged ion?

A

Anion

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14
Q

In giving valence electrons, the one with the least amount will give to the one with more, and the metal will give to the non-metal. True or False?

A

True

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15
Q

Who created the Lewis Dot Structure?

A

Gilbert Lewis

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16
Q

When doing the LEDS of an element, you should put one on all sides first before doubling the amount. True or False?

A

True

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17
Q

Is the ability of an atom to ACCEPT one or more electrons.

A

Electron Affinity

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18
Q

Is the ability of an atom to ATTRACT electrons.

A

Electronegativity

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19
Q

Both Electron Affinity and Electronegativity increase left then going down in the periodic table. True or False?

A

False. Both increase right then going up.

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20
Q

Chemical Bonding is the formation of a chemical bond to give rise to a chemical compound. True or False?

A

True

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21
Q

Ionic Bonding takes place between a?

A

Metal and Non-Metal

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22
Q

Covalent Bonding takes place between?

A

Two Non-Metals

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23
Q

What type of bonding leads to the formation of metals?

A

Metallic Bonding

24
Q

Solve for the electron configuration of Neon.

A

1s² 2s² 2p⁶

25
Q

Solve for the electron configuration of Phosphorus.

A

1s² 2s² 2p⁶ 3s² 3p³

26
Q

Solve for the electron configuration of Carbon.

A

1s² 2s² 2p²

27
Q

Solve for the electron configuration of Bromine.

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵

28
Q

FORMS OF COVALENT BONDING

1 pair of electrons shared

A

Single Bond

29
Q

FORMS OF COVALENT BONDING

2 pairs of electrons shared

A

Double Bond

30
Q

FORMS OF COVALENT BONDING

3 pairs of electrons shared

A

Triple Bond

31
Q

Why do Elements gain, lose, or share Valence Electrons?

A

To gain stability because of the Octet Rule.

32
Q

TYPES OF ORBITALS

Ending in s can only hold up to how many electrons?

A

2

33
Q

TYPES OF ORBITALS

Ending in p can only hold up to how many electrons?

A

6

34
Q

TYPES OF ORBITALS

Ending in d can only hold up to how many electrons?

A

10

35
Q

TYPES OF ORBITALS

Ending in f can only hold up to how many electrons?

A

14

36
Q

Non metal
Symbol = C
Atomic no. 6
4 valence electrons

A

Carbon

37
Q

Branch of chemistry in which we study carbon-containing compounds

A

Organic Chemistry

38
Q

Contains carbon, usually bonded to hydrogen
Covalent Bonding

Ex. Paper (cellulose), Nail Polish (nitrocellulose, butyl acetate), gasoline (mixed hydrocarbons), etc.\

A

Organic Compounds

39
Q

Usually don’t contain carbon
Ionic Bonding

Includes carbon dioxide, some carbonates, cyanides and carbides.

A

Inorganic Compounds

40
Q

Saturated Hydrocarbons

A

Single covalent bonds (alkane)

41
Q

Unsaturated Hydrocarbons

A

Double or triple bond (alkene or alkyne)

42
Q

1

A

Meth

43
Q

2

A

Eth

44
Q

3

A

Prop

45
Q

4

A

But

46
Q

5

A

Pent

47
Q

6

A

Hex

48
Q

7

A

Hept

49
Q

8

A

Oct

50
Q

9

A

Non

51
Q

10

A

Dec

52
Q

Single Bond

A

Alkane

53
Q

Double Bond

A

Alkene

54
Q

Triple Bond

A

Alkyne

55
Q

Based on chains of carbon atoms
Consists of linear, branched, straight-chained, and/or exist in cyclic structures
Can be saturated or unsaturated

A

Aliphatic

56
Q

Contains benzene or a heterocyclic ring

A

Aromatic

Grade 9 2nd Periodic Test (5 decks)

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