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Science - Periotic Table > Periodic Table test > Flashcards

Periodic Table test Flashcards

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1
Q

what is an atom and its structure?

A

an atom is the basic unit of matter, it is made up of three types of subatomic particles
1. protons
2. neutrons
3. electrons

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2
Q

What are protons?

A

Protons are positively charged particles that are found in the nucleus of an atom, they have a mass approximately 1 atoms mass unit (amu). the number of protons determines the atomic number.

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3
Q

What are neutrons?

A

Neutrons are neutral particles that are also found in the nucleus of an atom. they have a mass of approximately 1 amu.

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4
Q

What are electrons?

A

electrons are negatively charged particles that orbit the nucleus of an atom. they have a much smaller mass than protons and neutrons, approximately 1/1836 amu. The number of electrons are equal to the number of protons in an atom.

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5
Q

how do you calculate the number of neutrons in an element?

A

formula:
Number of neutrons = Atomic mas - Atomic number

Example: NA - Sodium
23 (round up from 22.99) - 11 = 12 –> this atom would have 12 neutrons

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6
Q

what are isotopes?

A

Isotopes are atoms of the same element that have the same amount of protons but a different number of neutrons.

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7
Q

Do isotopes have the same atomic number and atomic mass?

A

No, because of the different number of neutrons compared to protons the atomic number is different to the elements atomic mass.

Example:
Carbon 12 and carbon 14 are isotopes of carbon, they have 6 protons but 6 and 8 neutrons respectively.

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8
Q

Can isotopes be stable or radioactive?

A

Isotopes can be stable or radioactive and have different properties and uses depending on their stability and atomic mass.

This is why the mass number is not always a whole number, it is the average mass of all isotopes.

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9
Q

What are groups in the periodic table?

A

groups are arranged vertically and have similar chemical and physical properties. the elements in a group have the same number of valence electron.

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10
Q

What are valence electrons?

A

valence electrons are the electrons in the outermost shell that participate in chemical reactions. this is why elements in the same group have similar reactivity and form similar compounds.

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11
Q

What are periods in the periodic table?

A

periods are arranged horizontally and have elements with gradually increase atomic number.

the periods relate to the number of electron shells the atom has.

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12
Q

when moving across a period from the left to the right what happens

A

the atomic number of the element increases, and so does the number of protons, neutrons and electrons in the atom.

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13
Q

what is electron configuration?

A

Electron configuration relates to the group and rows of the periodic table.
1. the group number related to the number of valence electrons in the final shell.
2. the period number (or shell number) relates to the number of electron shells around the nucleus.

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14
Q

What is the final electron(s) in the last shell refer to?

A

the valence shell and the valence electron

this related to several key aspects of the periodic table such as their properties (reactivity) and location on the periodic table.

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15
Q

What is the maximum amount of electrons in a shell?

A

8
when one shell is full the remaining electrons will move to another shell.
each shell must be completed before moving to the next
this related to energy state of an atom

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16
Q

What is the maximum of electrons in the first shell?

A

2

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17
Q

What is the proton number in electrons and shells?

A

the proton number is equal to the number of electrons. e.g. MG has an atomic number of 12, hense it has 12 protons and 12 electrons.

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18
Q

what is the electronic configuration - notation for the element Li when the number of electrons is 3

A

2.1 –> because there is a total of 3 electrons, and the first shell can only hold a capacity of 2 electrons, the remaining electron(s) move to the net shell.
P=3 G=1

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19
Q

What is the electronic configuration - notation of Ca? the amount of elections is 20)

A

2.8.8.2

note: as you move down the periodic table they become more reactive

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20
Q

What are ions?

A

Ions are atoms that have lost or gained electrons which result in the atom being positively or negatively charged. this means it has an equal number of protons and electrons.

this changed the overall charge of the atom - either to positive or negative depending on it loosing or gaining an electron.

21
Q

Do atoms loose or gain protons?

A

no, only its electrons can be lost or gained

22
Q

How are the formation of ions based off?

A

The loss or gain of electrons to form an ion relates to which group the element is from the periodic table, specifically, the group number will determine how many electrons lost or gained.

23
Q

What are the two types of ions?

A

cations and anions

24
Q

What are Cations?

A

Cations are positively charged,formed by the loss of one or more electrons from an atom. they are formed when an atom loses electrons and becomes positively charged. They are metals.

25
Q

What are Anions?

A

Anions are negatively charged ions, formed by gaining one or more electrons by an atom. they are formed when an atom gains an electron and becomes negatively charged. They are non-metals.

26
Q

Why is it easier for an atom with one electron on the outer shell to become a cation?

A

because it is easier to lose 1 electron then there is gain 7 electrons to complete an electron shell.

27
Q

what is the definition of ionic bonding

A

a chemical bond between a metal and a non-metal. where one atom loses one or more electron/s, and the other atom gains one or more electron/s.
the metal becomes a cation because it looses electrons to the non-metal.

28
Q

how does a compound become neutrally charged?

A

The positively charged ion and negatively charged ion cancel each other out

29
Q

what happens when ionic bonding occurs?

A

the cations and anions are electrostatically attracted to each other forming a chemical bond.
when cations and anions bond together they create a neutral charge.

30
Q

how do you name ionic compounds?

A

the metallic (cation) compound will remain with its usual name, and the non-metal (anion) compound will keep its ‘root’ but will have the suffix ‘ide’ added to it.

31
Q

what is Na1+ and O2-

what is Mg2+ and H1-

A

Na1+ O2-
cross
2Na1O
Na2O
the two is on the bottom

Mg2+ H1-
cross
MgH2
the two is on the bottom

32
Q

what is the definition of covalent bonding

A

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

33
Q

what is the definition of metallic bonding

A

Metallic bonding is a type of chemical bond that happens between atoms in a metal.
Atoms bump into each other within the metal and share their electrons with each other.
The electrons that are shared move freely around the metal.
This is known as the ‘sea of electrons’.

34
Q

what are polyatomic atoms?

A

group of atoms that are chemically bonded together and have a net electric charge. These ions are formed by the combination of cations and anions. They are also known as molecular ions.

35
Q

where are alkali metals on the periodic table

A

group one

36
Q

what are the properties of alkali metals
give three

A

highly reactive’
soft
lustrous
high density
high thermal conductivity
low ionization energy
silvery-white color

37
Q

example of what an alkali metal is

A

phone screens are ductile to pick up electrical conductivity

38
Q

where are the alkali earth metals on the periotic table

A

group 2

39
Q

what are the properties of alkali earth metals
give three

A

highly reactive (less than g.1)
low ionization energy
harder than alkali metal
highly thermal conductivity
lower density than g.1
high thermal conductivity
form basic oxides when they react with oxygen.

40
Q

metalloid properties

A

luster: shiny appearance
semi-conductive: can conduct heat and electricity but not as good as metals
solid at room temperature
break easily - cannot be hammered or pressed

41
Q

example of a metalloid

A

the semi conductive nature allows electricity in the processer without overloading it.

42
Q

what are non-metals

A

a diverse group of elements that can be found across the perodic table. they have a wide range of properties.

43
Q

what are some of the characteristics of non-metals
give three

A

less reactive than metals
low ionization energy
varying physical states
poor conductors
high electron affinity
low desity and melting/boiling points
brittle and non lustrous

44
Q

where are halogens found on the periodic table?

A

group 7 (17)

45
Q

properties of halogens
give three

A

highly reactive
exist in different states
low melting/boiling points
high ionization energy
high electron affinity
will react with metal

46
Q

where are Nobel gases on the periodic table

A

group 8

47
Q

characteristics of Nobel gases

A

stable and do not react due to having a complete valence shell
colorless/odorless
exist in gases
low boiling points (easy to solidify and liquefy)
non-toxic

48
Q

draw the atomic structure of boron

A
49
Q

draw an atom

A

Science - Periotic Table (1 decks)

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