Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Hi gworll > Flashcards Deck 15229828 > Flashcards

Flashcards Deck 15229828

1
Q

Atoms have 3 subatomic particles. What are they?

A

Protons, Neutrons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Protons have a ___ charge

A

Positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Electrons have a _____ charge

A

Negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Neutrons have a ____ charge.

A

Neutral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What determines the atomic number?

A

The amount of protons in the atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What determines the atomic mass?

A

The average number of protons and neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why do certain elements have decimal places in their atomic mass?

A

Because they have different isotopes which can change their atomic mass which is why it calculated by the AVERAGE number of protons and neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are Isotopes?

A

Isotopes are atoms of the same element meaning they have the same number of protons but have slightly varying neutrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Isotopes can be reactive or stable. True or false?

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the group an element is in determine?

A

The number of electrons in the valence shell (the valence electrons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What does the period of an element represent?

A

The period of an element relates to the number of electrons shells the atom has

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are the properties of metals?

A

Ductile and malleable, good heat conductors, low ionisation levels causing them to be highly reactive and lustrous.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

The Metalloids include:

A

​Boron, Silicon, then numbers 32,33,51,52 and 84

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Non- metal properties include:

A

Poor conductors of heat and electricity, low melting and boiling points and brittle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The metalloids properties include:

A

Semi-conductive (they are okay, but are not as good as the metals), lustrous, often break easily, usually solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why are the noble gases called the noble gases?

A

They are stable due to having a complete valence shell, making them unreactive unless in very certain conditions .

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How many electrons can each electron shell fit?

A

The first one 2 and the rest 8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are ions?

A

Ions are atoms that have lost or gained electrons (never protons), changing the charge of the atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Cations= positive charged atoms

Anions= negatively charged atoms

True or false?

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Do Metalloids produce cations or anions?

A

None as they usually don’t form any ions.

21
Q

What ions do hydrogen produce?

A

Positive or negative. They can do both as it is equally easy for them to loose and gain an electron.

22
Q

How should the ionic charge be written?

A

1-/1+

23
Q

What is ionic bonding?

A

It is the chemical bond that forms between a metal and non-metal. The metal gives an electron to thr non metal, resultting the metal being a cation and the nonmetal being an anion.

24
Q

What is the charge of aluminium and Gallium?

A

+3

25
Q

Every one chlorine atom only needs 1 more electron to complete its electron shells yet magnesium needs to get rid of 2. What happens?

A

One magnesium atom needs to bond with 2 chlorine atoms

26
Q

1 magnesium atom for every 2 chlorine atom. How would you write this?

A

MgCl2

27
Q

What is the ionization energy?

A

The amount of energy required to remove an electron from an atom

28
Q

What are common patterns in ionic compounds?

A

The ends of our anions sometimes change to -ide or -ite

29
Q

What is a Polyatomic ion?

A

It is a group of atoms that have chemically bonded to create an ion.

30
Q

What is Metallic bonding?

A

A type of chemical bonding that happens between metals where one arr more atoms will share electrons with eachother. This means the electrons will be able to move freely between the cations, creating a sea of electrons.

31
Q

How does electricity power through metal’s that are metallicaly bonded.

A

The reason metals conduct heat so well is because the electrons in them can move around easily, and they can carry heat from one part to another. Metal atoms are packed more densely and can transmit heat vibrations more readily.

32
Q

How are metalls malleable?

A

Metals are malleable because the ions in their lattice structure can slide over one another without breaking apart as the ions are not stuck together, but rather are held in close proximity by their attraction to the sea of electrons around them.

33
Q

What is Covalent bonding?

A

When non-metal atoms share electrons with each other in order to achieve a full valence shell of electrons and become more stable.

34
Q

How are electrons shared in metallic bonding?

A

Usually in pairs (1 electron each, 2 electrons each ect.)

35
Q

Covalent bonds Form both simple and complex molecules. True or false

A

True

36
Q

What state are Covalent bonded molecules in? Liquid gas or solid?

A

Gases or liquid.

37
Q

What are the properties of covalent bonded molecules?

A

They are poor conductors of heat and electricity and also have a low boiling and melting point.

38
Q

Reactivity of atoms in group 1 and 2 increases the further ____________ you go.

A

Left and downward

39
Q

Which elements are most similar to each other?

A

Those in the same group, or column of the periodic table because they have the same number of valence electrons

40
Q

Why do atoms ionize?

A

To achieve a full valence shell in order to be stable

41
Q

What is another name for a molecular ion?

A

A Polyatomic ion.

42
Q

What state do noble gasses exist in at room temperature?

A

Gas

43
Q

Reactivity of atoms in group 6 and 7 increases the further ____________ you go.

A

Right and upward

44
Q

What does Monatomic mean?

A

A molecule composed of just one atom, and lacking any covalent bonds- usually the noble gasses

45
Q

What does diatomic mean?

A

Molecules composed of only two atoms, of the same or different chemical elements.

46
Q

Are metals cations or anions?

A

Cations- they lose an electron, being more positively charged

47
Q

Are non-metals cations or anions

A

Anions- they gain an electron, being more Negatively charged

48
Q

Can the alkali metals, alkaline earth metals and Halogens ever exist as monatomic in nature?

A

Usually not naturally, while they can be found like that in a lab, they are usually seen bonded either through ionic, covalent or metallic bonding.

Hi gworll (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions