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Size & Mass of Atoms Name Name: 5.1.1.5 – Size & Mass of Atoms Date / / Keywords 1. Starter: How small is an atom? 3. Label the atom using the keywords Atom Radius - Nucleus + Protons + Neutrons Electrons - Shells Mass Number 2. How small is an atom? 4. How small is the nucleus of the atom? Atomic Number An atom has a ________ of about _____ • The radius of the _________ is less than ___/__________ of the atom. Element This means the atom is mostly _________ __________. nm stands for _________________ Isotope • However, almost all of the ________ of the atom comes from the nucleus. 6. How to work out the number of neutrons. This means almost all of the mass comes from the _________ and _________. We can work out the number of neutrons by subtracting the ________ ________ from the _________ ________. 5. Atomic Number & Mass Number 7 4 Work out the number of neutrons in lithium: This tells us the _____ of the atom which comes from the ________ + ________ in the nucleus - Li 7 – 3 = ____ Neutrons. He 3 2 This tells us the number of ___________ in the nucleus which is the same as the number of negative ________. 7. Work out the number of protons, neutrons and electrons for each element: 9. Isotopes 4 7 31 Elements with the same number of Protons ______ Protons ______ Protons ______ _______ and _________, but Neutrons _____ Neutrons _____ Neutrons _____ He Li P different numbers of _________ 2 Electrons _____ 3 Electrons _____ 15 Electrons _____ are called ___________. 23 20 80 Protons ______ Protons ______ Protons ______ Feedback Neutrons _____ Neutrons _____ Neutrons _____ Na Ne Br Electrons _____ Electrons _____ 11 Electrons _____ 10 35 18 8. Work out the number of protons, neutrons and electrons for each element: 35 Protons ______ 37 Protons ______ Neutrons _____ Neutrons _____ Cl Cl 17 Electrons _____ 17 Electrons _____ Q1. Why are they the same element? Both are the element ________ as they both have ____ protons. Q2. What is the same about them? They have the same number of _________ and __________ Q3. What is different about them? They have different numbers of ___________, this makes them _____________ The Size & Mass of atoms 5.1.1.5 5.1.1.5 - Students should be able to: State that atoms a very small, with a radius of 0.1 nm Explain that the nucleus of an atom is even smaller = 1/10,000 the radius of the atom. Describe how almost all of the mass of the atom is concentrated in the nucleus with the protons and neutrons. Define mass number and atomic number. State that the element is defined by the atomic number. Calculate the number of protons, neutrons and electrons in an atom. Explain what isotopes of an element are. How small is an atom? • Write down how small you think an atom is on a post-it. • You could use a comparison to another object…. • Or you could use units, e.g. meters… (m) How small is an atom? • Atoms are very small, they have a radius of about 0.1 nm • That’s 1 x 10-10 m ! Task: Label the atom Electron Keywords Proton - 1. Proton 2. Neutron Nucleus + Shell 3. Electron + 4. Nucleus 5. Shell Neutron - How big is the nucleus compared with the whole atom? How small is the nucleus compared with the whole atom? The radius of a nucleus is less than 1/10,000 of the atom! But the nucleus makes up almost all the mass of an atom! nucleus Therefore: which particles . are responsible for the mass of the atom? Recap • Atoms are very small. • The radius of an atom is 0.1nm (small!) • The radius of the nucleus is 1/10,000 the radius of the atom (even smaller!) • Almost all the mass of the atom comes from its tiny nucleus. • The nucleus contains protons and neutrons. Atomic number & Mass number On the periodic table we find elemental symbols like this: The largest number is called the “mass number” Mass number There are two numbers, one above This number tells us the mass of an atom of this element. the other below: Q. Where4 does almost all the mass of the atom come from? The nucleus! Q. What particles were in the nucleus? Protons & Neutrons! He Q. So what does the mass number also tells us? The sum of2 (protons + neutrons) Mass number 2 protons + 2 neutrons = mass number of 4 So why is Heliu’s ass uber = 4? 2 x Proton - 4 Nucleus + He + 2 2 x Neutron - Mass Number Recap • Almost all the mass of an atom comes from the nucleus. • The nucleus contains protons and neutrons. • When you add up the numbers of protons and neutrons you get the mass of the atom! • This is called the “Mass number” Atomic Number • The atomic number tells us the number of ______________Protons • Which is the same as the number of _________Electrons Atoms have an equal number of positive - protons and negative 4 electrons. This is so the atom has no overall electrical charge. + He + 2 Atomic Number - Look at the periodic table, what do you notice about the numbers? Key fact! 1 4 7 9 H He Li Be 1 2 3 4 • The number of protons defines the element! • Elements are arranged on the periodic table in order of their atomic numbers. • If you change the number of protons (atomic number) you change the element! Mass number Mass number 4 Protons + Neutrons So how do we work out the number of neutrons? He Mass number – atomic number = number of neutrons. 4 – 2 = 2 neutrons. 2 Atomic number Atomic number Protons Practice: Protons, Neutrons and Electrons Key maths skill 2 15 4 Protons ______ 7 Protons ______3 31 Protons ______ Neutrons _____2 Neutrons _____4 Neutrons _____16 He Li P 2 3 15 2 Electrons _____ 3 Electrons _____ 15 Electrons _____ 11 10 35 23 Protons ______ 20 Protons ______ 80 Protons ______ Neutrons _____12 Neutrons _____10 Neutrons _____45 Na Ne Br 11 10 35 11 Electrons _____ 10 Electrons _____ 35 Electrons _____ Calculate protons, neutrons and electrons for both. 17 35 Protons ______ 37 Protons ______17 Neutrons _____18 Neutrons _____20 Cl Cl 17 17 17 Electrons _____ 17 Electrons _____ Q1. Why are they the same element? Both are chlorine as they both have 17 protons. Q2. What is the same about them?ISOTOPES They have the same number of protons (17) and electrons (17). A version of an element with a different number of neutrons, Q3. What is different aboutbut the them? same numberThey have of different protons numbers and electrons. of neutrons! One has 18, the other has 20 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca B C Electron configuration Name: The golden rules: First you need to count the number of _______________, you can get this from the element’s ________ _________. The first shell can take a maximum of _________ electrons. All other shells can take up to ___________ electrons. Draw the electron configuration for sodium (Na) and Oxygen (O): Sodium has 11 electrons, Oxygen has 8 electrons. Na O ____, ____, _____ _____, ____ How elements are arranged on the periodic table Lithium (Li), Sodium (Na) and Potassium (K) are all in group ____ because they all have ____ electron in their outer shells. Beryllium (Be), Magnesium (Mg) and calcium (Ca) are all in group ____ because they all have ____ electron in their outer shells. Fluorine (F), Chlorine (Cl) and Bromine (Br) are all in group ____ because they all have ____ electron in their outer shells. Helium (He), Neon (Ne) and Argon (Ar) are all in group ____ because they all have ____ electron in their outer shells. Elements in the same group ________ similarly because they have the same number of _________ in their outer shells. Elements in group ___ are very _____________ because they have _______ outer shells. Electron configuration Name: The golden rules: First you need to count the number of _______________, you can get this from the element’s _________ ________. The first shell can take a maximum of _________ electrons. All other shells can take up to ___________ electrons. Draw the electron configuration for sodium (Na) and Oxygen (O): Sodium has 11 electrons, Oxygen has 8 electrons. Na O ____, ____, _____ _____, ____ How elements are arranged on the periodic table Lithium (Li), Sodium (Na) and Potassium (K) are all in group ____ because they all have ____ electron in their outer shells. Beryllium (Be), Magnesium (Mg) and calcium (Ca) are all in group ____ because they all have ____ electron in their outer shells. Fluorine (F), Chlorine (Cl) and Bromine (Br) are all in group ____ because they all have ____ electron in their outer shells. Helium (He), Neon (Ne) and Argon (Ar) are all in group ____ because they all have ____ electron in their outer shells. Elements in the same group ________ similarly because they have the same number of _________ in their outer shells. Elements in group ___ are very _____________ because they have _______ outer shells. Name: ______________________________ 5.1.1.6 - Electronic Structure Class: ______________ Date: ____/____/_________ Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 Group 0 1 4 H He 1 2 H He Period 1 Period __ __ 7 9 11 12 14 16 19 20 Li Be B C N O F Ne 3 4 5 6 7 8 9 10 F Ne Li Be B C N O Period 2 Period __,__ __,__ __,__ __,__ __,__ __,__ __,__ __,__ 23 24 27 28 31 32 35.5 40 Na Mg Al Si P S Cl Ar 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar Period 3 Period __,__,__ __,__,__ __,__,__ __,__,__ __,__,__ __,__,__ __,__,__ __,__,__ 39 40 • Electrons are represented by _____ K Ca 19 20 • Electrons will occupy the lowest available _________ ________.
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